Chemistry MC: December 2018

Archive for December 2018

How much energy (in kJ) do 3.0 moles of photons all with a wavelength of 655 nm, contain?

A) 183 kJ
B) 303 kJ
C) 394 kJ
D) 548 kJ
E) 254 kJ

Answer: D

How many photons are contained in a flash of green light (525 nm) that contains 189 kJ of energy?

A) 5.67 × 1023 photons
B) 2.01 × 1024 photons
C) 1.25 × 1031 photons
D) 4.99 × 1023 photons
E) 7.99 × 1030 photons

Answer: D

How many photons are contained in a burst of yellow light (589 nm) from a sodium lamp that contains 609 kJ of energy?

A) 3.37 × 1019 photons
B) 3.06 × 1030 photons
C) 1.80 × 1024 photons
D) 4.03 × 1028 photons
E) 2.48 × 1025 photons

Answer: C

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.

A) 4.85 × 10-19 J
B) 2.06 × 10-19 J
C) 1.23 × 10-19 J
D) 8.13 × 10-19 J
E) 5.27 x 10-19 J

Answer: A

Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm.

A) 3.54 × 10-19 J
B) 4.27 × 10-19 J
C) 2.34 × 10-19 J
D) 6.45 × 10-19 J
E) 2.83 × 10-19 J

Answer: E

Which of the following occur as the wavelength of a photon increases?

A) the frequency decreases
B) the energy increases
C) the speed decreases
D) Planck's constant decreases
E) None of the above occur as the wavelength of a photon increases.

Answer: A

Which of the following occur as the energy of a photon increases?

A) the frequency decreases.
B) the speed increases.
C) the wavelength increases
D) the wavelength gets shorter.
E) None of the above occur as the energy of a photon increases.

Answer: D

Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 486.1 nm.

A) 1.46 × 1014 s-1
B) 6.86 × 1014 s-1
C) 4.33 × 1014 s-1
D) 6.17 × 1014 s-1
E) 1.62 × 1014 s-1

Answer: D

Calculate the energy of the orange light emitted per photon, by a neon sign with a frequency of 4.89 × 1014 Hz.

A) 3.09 × 10-19 J
B) 6.14 × 10-19 J
C) 3.24 × 10-19 J
D) 1.63 × 10-19 J
E) 5.11 × 10-19 J

Answer: C

Calculate the energy of the green light emitted per photon, by a mercury lamp with a frequency of 5.49 × 1014 Hz.

A) 2.75 × 10-19 J
B) 3.64 × 10-19 J
C) 5.46 × 10-19 J
D) 1.83 × 10-19 J
E) 4.68 × 10-19 J

Answer: B

Calculate the frequency of the red light emitted by a neon sign with a wavelength of 659.9 nm.

Calculate the frequency of the red light emitted by a neon sign with a wavelength of
659.9 nm.

A) 2.20 × 1014 s-1
B) 1.98 × 1014 s-1
C) 4.55 × 1014 s-1
D) 5.05 × 1014 s-1
E) 3.32 × 1014 s-1

Answer: C

Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz.

A) 229 nm
B) 436 nm
C) 206 nm
D) 485 nm
E) 675 nm

Answer: B

Calculate the wavelength (in nm) of a the red light emitted by a neon sign with a frequency of 4.74 × 1014 Hz.

A) 633 nm
B) 158 nm
C) 142 nm
D) 704 nm
E) 466 nm

Answer: A

Which of the following types of electromagnetic radiation has the smallest frequency?

A) yellow
B) blue
C) orange
D) green
E) purple

Answer: C

Which of the following types of electromagnetic radiation has the shortest wavelength?

A) blue
B) violet
C) orange
D) green
E) yellow

Answer: B

Which of the following visible colors of light has the longest wavelength?

A) blue
B) green
C) yellow
D) red
E) violet

Answer: D

Which of the following visible colors of light has the largest frequency?

A) green
B) red
C) blue
D) yellow
E) orange

Answer: C

Identify the color that has a wavelength of 460 nm.

A) blue
B) green
C) red
D) yellow

Answer: A

Identify the color that has a wavelength of 700 nm.

A) blue
B) green
C) red
D) yellow

Answer: C

Place the following types of electromagnetic radiation in order of decreasing energy. ultraviolet light radio waves microwaves

Place the following types of electromagnetic radiation in order of decreasing energy.
ultraviolet light radio waves microwaves

A) radio waves > microwaves > ultraviolet light
B) ultraviolet light > microwaves > radio waves
C) radio waves > ultraviolet light > microwaves
D) ultraviolet light > radio waves > microwaves
E) microwaves > radio waves > ultraviolet light

Answer: B

Place the following types of electromagnetic radiation in order of increasing frequency. visible light microwaves X-rays

Place the following types of electromagnetic radiation in order of increasing frequency.
visible light microwaves X-rays

A) microwaves < visible light < X-rays
B) X-rays < visible light < microwaves
C) microwaves < X-rays < visible light
D) X-rays < microwaves < visible light
E) visible light < X-rays < microwaves

Answer: A

Place the following types of electromagnetic radiation in order of increasing wavelength. ultraviolet light gamma rays radio waves

Place the following types of electromagnetic radiation in order of increasing wavelength.
ultraviolet light gamma rays radio waves

A) gamma rays < radio waves < ultraviolet light
B) radio waves < ultraviolet light < gamma rays
C) radio waves < gamma rays < ultraviolet light
D) ultraviolet light < gamma rays < radio waves
E) gamma rays < ultraviolet light < radio waves

Answer: E

A hydrogen atom absorbs a photon of UV light and its electrons enter the n =4 energy level. Calculate the change in energy of the atom and the wavelength (in nm) of the photon.

Answer:

2.04 X 10^-18 J
97.4 nm

Green light has a wavelength of 5200 A. Calculate the energy of one photon of green light.

Answer: 3.8 x 10^-19 J (E = hc/wavelength)

Infrared radiation from the the sun has a wavelength of 6200 nm. Calculate the energy of one photon of that radiation?

Answer: between 10^-20 and 10^-19 (E = hc/wavelength)

A radio has a frequency of 8.6 X 10^8 Hz. What is the energy of one photon of this radiation?

Answer: 5.7 x 10^-25 J (E = hv =hc/wavelength)

A cook uses a microwave oven to heat a meal. The wavelength of the radiation is 1.20 cm. What is the energy of one photon of this microwave oven?

Answer: 1.66 X 10^-23 J (E = hv = hc/wavelength)

Yellow light has a frequency of 5.2 x 1014 s -1 while red light has a frequency of 4.3 x 1014 s -1 . Which of the following correctly describes the relationship between the wavelength and energy of yellow versus red light?

(a) Red light has a longer wavelength and more energy than yellow light.
(b) Yellow light has a longer wavelength and more energy than red light.
(c) Red light has a longer wavelength and less energy than yellow light.
(d) Yellow light has a longer wavelength and less energy than red light.
(e) None of these.

Answer: (c) Red light has a longer wavelength and less energy than yellow light.

The energy of the electron of a hydrogen atom in the ground (n = 1) state is ___________.

(a) -2.18 × 10-18 J
(b) +2.18 × 10-18 J
(c) -1.64 × 10-19 J
(d) +1.64 × 10-19 J
(e) 0 (zero)

Answer: (a) -2.18 × 10-18 J

What is the wavelength of a neutron (the mass of a neutron is 1.675 × 10-27 kg) traveling at 100.0 m/s?

(a) 1.79 × 10-29m
(b) 1.32 × 10-15 m
(c) 3.96 × 10-9 m
(d) 2.53 × 108 m
(e) 5.97 × 1026 m

Answer: (c) 3.96 × 10-9 m

Which equation represents the electron affinity (E.A.) of the tungsten (W, 74) atom?

(a) W ➞ W+1 + e-
(b) W-1 ➞ W + e-
(c) W+1 + e- ➞ W-1 + e+
(d) W + e- ➞ W-1
(e) W+1 + e- ➞ W

Answer: (d) W + e- ➞ W-1

Given the information below, what is the average valence electron energy for the oxygen atom (O, 8)? Ionization Energies (in unites of MJ/mol) Element 1s 2s 2p O 52.6 3.12 1.31

(a) 1.44 MJ/mol
(b) 1.91 MJ/mol
(c) 14.6 MJ/mol
(d) 19.4 MJ/mol
(e) 116.7 MJ/mol

Answer: (b) 1.91 MJ/mol

Which of the following atoms or ions is the smallest?

(a) O2- (8)
(b) Na (11)
(c) Na+
(d) Mg (12)
(e) Mg2+

Answer: (e) Mg2+

Arrange the following four atoms in order from smallest to largest radius: Fluorine (F, 9); Neon (Ne, 10); Sodium (Na, 11); Magnesium (Mg, 12)

(a) F < Ne < Na < Mg
(b) Mg < Na < Ne < F
(c) Ne < F < Mg < Na
(d) Na < Mg < F < Ne
(e) Ne < Mg < F < Na

Answer: (c) Ne < F < Mg < Na

Which of the following atoms contains the most unpaired electrons in its ground state?

(a) B (5)
(b) N (7)
(c) Cl (17)
(d) Ti (22)
(e) Cu (29)

Answer: (b) N (7)

Which electron configuration of p orbitals would satisfy Hund's rules?

(a) ↓ ↓ ↓
(b) ⇅
(c) ⇈ ↑ ↑
(d) ⇵ ↑ ↓
(e) None of these configurations satisfy Hund's rules.

Answer: (a) ↓ ↓ ↓

What -2 ion can have an electron configuration of 1s2 2s2 2s6 3s1 3p1 ?

(a) F (9)
(b) Ne (10)
(c) Na (11)
(d) Mg (12)
(e) Al (13)

Answer: (b) Ne (10)

What is the correct electron configuration for the zirconium (Zr, 40) atom?

(a) [Kr] 5s 1 3d3
(b) [Kr] 5s 2 3d2
(c) [Kr] 4d4
(d) [Kr] 5s1 4d3
(e) [Kr] 5s2 4d2

Answer: (e) [Kr] 5s2 4d2

A possible set of quantum numbers for the last electron added to form a gallium atom (Ga, 31) in its lowest energy state is:

(a) 3, 1, 0, -½
(b) 3, 2, 1, +½
(c) 4, 0, 0, +½
(d) 4, 1, 1, +½
(e) 4, 2, 2, +½

Answer: (d) 4, 1, 1, +½

The Pauli exclusion principle states that:

(a) No two electrons in an atom can have the same spin.
(b) No two electrons in an atom can occupy the same orbital.
(c) Two electrons in the same orbital have identical values of the spin quantum number.
(d) No two electrons in an atom can have the same set of four quantum numbers.
(e) Electrons in a subshell are arranged to maximize the total amount of spin.

Answer: (d) No two electrons in an atom can have the same set of four quantum numbers.

In a single atom, what is the maximum number of electrons could have a principal quantum number (n) of 4 and an angular quantum number (l) of 1?

(a) 2
(b) 6
(c) 8
(d) 10
(e) 18

Answer: (b) 6

Which of the following quantum numbers is used to describe the orientation of an orbital in space?

(a) The principal quantum number, n
(b) The angular quantum number, l
(c) The magnetic quantum number, ml
(d) The spin quantum number, ms
(e) None of these quantum numbers describe the orientation of an orbital in space.

Answer: (c) The magnetic quantum number, ml

Which of the following elements requires the most energy to remove its most tightly held electron (the electron closest to the nucleus): Magnesium (Mg, 12); Aluminum (Al, 13); Silicon (Si, 14); Phosphorus (P, 15); Sulfur (S, 16)

(a) Mg
(b) Al
(c) Si
(d) P
(e) S

Answer: (e) S

Which element is represented by the following PES spectrum?

(a) Sc (21)
(b) Ti (22)
(c) V (23)
(d) Cr (24)
(e) Mn (25)

Answer: (d) Cr (24)

An atom in its ground state absorbs two photons: a photon with a wavelength of 102.6 nm and then a photon with a wavelength of 1875 nm. The atom then relaxes back to the ground state by emitting a single photon. What is the wavelength of the emitted photon?

(a) 18.38 nm
(b) 97.25 nm
(c) 108.5 nm
(d) 1772 nm
(e) 1977 nm

Answer: (b) 97.25 nm

The first ionization energy of the first six elements in the periodic table is given below. H 1312.0 kJ/mol He 2372.3 Li 520.2 Be 899.4 B 800.6 C 1086.4 Why is the first ionization energy of B smaller than Be?

(a) Because the first IE tends to decreases as we go across a row of the periodic table from left to right.
(b) Because the nucleus of a B atom contains fewer protons than the nucleus of a Be atom.
(c) Because the outermost electron on B is in a 2p orbital, while in Be it is in a 2s orbital.
(d) Because the atomic number of B is odd, whereas the atomic number of Be is even.
(e) Because B has orbitals containing paired electrons while Be does not.

Answer: (c) Because the outermost electron on B is in a 2p orbital, while in Be it is in a 2s orbital.

Arrange the following elements in order of increasing first ionization energy: Sulfur (S, 16); Argon (Ar, 18); Calcium (Ca, 20)

(a) S < Ar < Ca
(b) Ar < S < Ca
(c) Ca < Ar < S
(d) S < Ca < Ar
(e) Ca < S < Ar

Answer: (e) Ca < S < Ar

Which of the following transitions from a hydrogen atom with an electron in the n = 5 state will result in the emission of the longest wavelength of light?

(a) n = 5 ➞ n = 0
(b) n = 5 ➞ n = 1
(c) n = 5 ➞ n = 4
(d) n = 5 ➞ n = 6
(e) n = 5 ➞ n = ∞

Answer: (c) n = 5 ➞ n = 4

The line structure of the emission spectrum of the hydrogen atom suggests that:

(a) The atom is composed of a small positive nucleus and electrons.
(b) There are many electrons in a hydrogen atom.
(c) The position and energy of an electron cannot be determined simultaneously.
(d) The energies of electrons are quantized.
(e) Each electron has multiple energies.

Answer: (d) The energies of electrons are quantized.

What is the wavelength, in meters, of light that has a frequency of 2.33 x 1015 s -1 ?

(a) 6.99 x 1023 m
(b) 7.77 x 102 m
(c) 7.77 x 106 m
(d) 12.9 m
(e) 1.29 x 10-7 m

Answer: (e) 1.29 x 10-7 m

If X-rays have a shorter wavelength than ultraviolet light, which of the following statements is true?

(a) X-rays have smaller frequencies than UV light.
(b) X-rays travel faster than UV light.
(c) X-rays have more energy than UV light.
(d) X-rays have larger amplitudes than UV light.
(e) Both answers (a) and (c)

Answer: (c) X-rays have more energy than UV light.

What is the frequency of radiation of wavelength 810 nm?

Answer:

so 810 nanometer = 810 X 10^-9
velocity of light = vel of radiations = 3X10^8 m/s.
so frequency=Velocity/Wavelength
=(3.0 X 10^8)/(8.10 X 10^-11).
=3.7X10^14

How many photons are in a 1.20mJ burst of this radiation?

Answer: (1.210^-3)/6.0210^-19=1.99*10^15

If the 330 nm radiation provides exactly the energy to break an average chemical bond in the skin, estimate the average energy of these bonds in kJ/mol.

Answer: 3.63x10^5 J/1000=363

One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 330 nm .What is the energy of a photon of this wavelength?

Answer:

Ephoton = (h x c) / Lambda
Ephoton = ((6.63x10^-34) x (3x10^8)) / (330x10^-9)
Ephoton = 6.03x10^-19 J

Which of the following statements concerning experiment and explanation is/are true?

1. A law is always given in the form of a mathematical expression.
2. Once a hypothesis passes one or two tests it is considered a theory.
3. Observation is a key component of the scientific method.

A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1,2, and 3

Answer: C) 3 only

Which nuclide has the same number of protons as ¹⁴₇N?

A) ¹⁹₉F
B) ¹⁵₇N
C) ¹⁵₈O
D) ³¹₁₅P
E) ¹²₆C

Answer: B) ¹⁵₇N

The property of a series of repeated measurements that is most directly related to precision is

A) the number of place holders in each measurement.
B) the accuracy of each measurement.
C) the reproducibility of each measurement.
D) the number of significant figures in each measurement.
E) the exactness of each measurement.

Answer: C) the reproducibility of each measurement.

An ion is formed

A) by either adding neutrons to or subtracting neutrons from the atom.
B) by either adding protons to or subtracting protons from the atom.
C) by either adding electrons to or subtracting electrons from the atom.
D) All the above are true.
E) Two of the above are true.

Answer: C) by either adding electrons to or subtracting electrons from the atom.

Which of the following conclusion regarding Rutherford's gold foil experiment is not consistent with the observations?

A) The nucleus occupies a large amount of the atom space.
B) The nucleus occupies only a small portion of the space of an atom.
C) Wide angle deflections result from a collision of an alpha particle and a gold atom nucleus.
D) The nucleus, like the alpha particles used to bombard the gold foil, is positively charged.
E) Most alpha particles travel straight through the gold foil.

Answer: A) The nucleus occupies a large amount of the atom space.

A sample that cannot be separated into two or more substance by physical means is

A) a homogeneous mixture.
B) a heterogeneous mixture.
C) either a compound or an element.
D) en element.
E) a compound.

Answer: C) either a compound or an element.

A sample of silicon is burned in oxygen to form silicon dioxide. What mass of oxygen is consumed if 57.76 g silicon dioxide is formed from 27.00 g silicon?

A) .47 g
B) 30.76 g
C) 84.76 g
D) 1559.59 g
E) none of the above.

Answer: B) 30.76 g

6.7 kilogram(s) contains this many grams:

A) 6.7 × 10⁻³
B) 6.7 × 10³
C) 0.67
D) 6.7 × 10²
E) 67

Answer: B) 6.7 × 10³

How many oxygen atoms are there in a formula unit of UO₂(C₂H₃O₂)₂ • NH₄C₂H₃O₂ • 4H₂O?

A) 12
B) 4
C) 10
D) 8
E) 21

Answer: A) 12

Cathode rays are

A) anions.
B) electrons.
C) cations.
D) protons.
E) positrons.

Answer: B) electrons.

Neon has three naturally occurring isotopes. The abundance of ²⁰Ne is 90.48% and ²²Ne is 9.25%. What is the percent abundance of ²¹Ne?

A) 49.9%
B) 9.25%
C) 33.2%
D) 81.2%
E) 0.27%

Answer: E) 0.27%

According to the law of multiple proportions:

A) if the same two elements form two difference compounds, they do so in a the same ratio.
B) it is not possible for the same two elements to form more than one compound
C) the ratio of the masses of the elements in a compound is always the same.
D) the total mass is the same after a chemical change as before the change.
E) None of these.

Answer: E) None of these.

The average speed of oxygen molecules at 690°C is 1.60 × 10⁵ cm/s. Which of the following calculations would convert this speed to units of miles per hour?

A) (1s/1.6 × 10⁵ cm) × (2.54 cm/1 in) × (1 ft/12 in) ×
(1 mi/5280 ft) × (3600s/1 h)

B) (1s/1.6 × 10⁵ cm) × (2.54 cm/1 in) × (12 in/1 ft) ×
(5280 ft / 1 mi) × (1 h/3600s)

C) (1.6 × 10⁵ cm/1s) × (2.54 cm/1 in) × (12 in/1 ft) ×
(5280 ft / 1 mi) × (3600s/1 h)

D) (1.6 × 10⁵ cm/1s) × (1 in/2.54 cm) × (1 ft/12 in) ×
(1 mi/5280 ft) × (3600s/1 h)

E) (1.6 × 10⁵ cm/1s) × (1 in/2.54 cm) × (12 in/1 ft) ×
(5280 ft / 1 mi) × (1 h/3600s)

Answer: D) (1.6 × 10⁵ cm/1s) × (1 in/2.54 cm) × (1 ft/12 in) × (1 mi/5280 ft) × (3600s/1 h)

Choose the group containing the most reactive nonmetals.

A) Group 8A
B) Group 3A
C) Group 1A
D) Group 5A
E) Group 7A

Answer: E) Group 7A

What is the volume of a cube that has an edge length of 0.019 m?

A) 6.9 cm³
B) 6.9 × 10⁻³ cm³
C) 6.9 × 10⁻³ m³
D) 6.9 × 10⁻³ km³
E) 6.9 × 10⁻³ mm³

Answer: A) 6.9 cm³

In a particular mass of KAu(CN)₂, there are 8.87×10²⁰ atoms of gold. What is the total number of atoms in this sample?

A) 2.66 × 10²¹
B) 1.77 × 10²¹
C) 5.32 × 10²¹
D) 3.55 × 10²¹
E) 4.44 × 10²¹

Answer: C) 5.32 * 10²¹

A species that is formed when a molecule gains or loses an electron is called

A) an ion.
B) an atom.
C) an isotope.
D) a metalloid.
E) a metal

Answer: A) an ion.

Which of the following statement concerning the SI system is/are correct?

1. Prefixes are used to indicate a power of ten multiplier for a given SI base unit of measurement.
2. Degrees Celsius(°C) is the SI base unit for temperature.
3. The kilogram (kg) is the SI base unit for mass

A) 1 only
B) 2 only
C) 3 only
D) 1 and 3
E) 1,2,and 3

Answer: D) 1 and 3

A 4.06 cm³ sample sodium metal has a a density of 0.968 g/cm³. What volume does this sample of sodium occupy in its liquid state? The density of liquid sodium is 0.927 g/cm³.

A) 4.24 cm³
B) 0.257 cm³
C) 3.64 cm³
D) 3.89 cm³
E) 4.52 cm³

Answer: A) 4.24 cm³

How many molecules of phosphoric acid (H3PO4) react with excess calcium carbonate (CaCO3) to produce 25.0 g of Ca3(PO4)2?

Answer: 9.72x10 to the 22nd mc H3PO4 react with CaCO3 producing 25 g of Ca3(PO4)2.

An organic compound methyl acrylate consists of 65.80% C, 37.17% O, and the rest Hydrogen (7.03%). If the molar mass of methyl acrylate is 86.1 g what are its empirical and molecular formulas?

Answer:

Empirical: C2OH3
Molecular: C4O2H6

How many moles of Caffeine are in a 10g sample?(Hint: 194.2=1 mol).

Answer: 0.05 mol in 10g sample

Calculate he molar mass of Caffeine (C8H10N4O2).

Answer: 194.2 g

A 3.0 mol sample of KClO3 was decomposed according to the equation 2KClO3 (s)-> 2KCl (s) + 3O2. How many moles of O2 are formed assuming 100% yield.

Answer: 4.5 mol

Which represents the greatest number of atoms?

1) 50.0 g of Al
2) 50.0 g of Cu
3) 50.0 g of Zn
4) 50.0 g of Fe
5) None of the Above

Answer: 1) 50.0 g of Al

Consider the equation 2A + B -> A2B If you react 1.0 mol of A with 1.0 mil of B, how much A2B can be produced?

Consider the equation 2A + B -> A2B
If you react 1.0 mol of A with 1.0 mil of B, how much A2B can be produced?

Answer: 0.50 mol

The empirical formula of styrene is CH; its molar mass is 104.1g/ mol. What is the molecular formula of styrene?

Answer: C8H8

What is the mass of one mole of copper in grams?

Answer: 63.5 g

The _____ equation contains all ions and substances that are in a reaction in aqueous solution.

Answer: Complete Ionic

When a precipitate reaction occurs the ions that do not form the precipitate

1) evaporate
2)are cations only
3) form insoluble solution
4) left to dissolve
5) none of these

Answer: 5) none of these

The spectator ion in the reaction Zn(NO3)2+2NH4OH -> 2NH4NO3 + Zn(OH)2 are:

Answer: NH4 and NO3

Based on the activity series the reaction that is most likely to occur from among the following is:

1) Ni+ BaNO3
2) Cu + HNO3
3) Pb + Na2SO4
4) Mg + HCl

Answer: 4) Mg+HCl

The most common factors that cause chemical reactions to occur are all the following except:

1) Formation of a solid
2) formation of a gas
3) formation of water
4) transfer of electrons
5) decrease in temperature

Answer: 5) decrease in temperature

In an oxidation reduction reaction:

Answer: The reactants are usually a metal and a nonmetal

In a precipitation reaction:

Answer: The reactants are generally two ionic compounds in aqueous solution

Identify the solid that forms when the following aqueous solutions are mixed: KNO3 (aq) + BaCl2 (aq)->

Answer: None Forms

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrates. The balanced complete ionic equation contains which correct coefficient and ion.

Answer: 2Ag+ (aq)

You have exposed electrodes of a lightbulb in a solution of H2SO4 so that the lightbulb is on. You add a dilute solution and the bulb goes dim. Which did you add?

1) Ba(OH)2
2)NaNO3
3)K2SO4

Answer: 1) Ba(OH)2

Which of the following compounds is soluble in water?

1) Fe(OH)2
2) Mg3(PO4)2
3) Sr(SO4)2
4) Na2CO3
5) PbCl2

Answer: 4) Na2CO3

Write the formula for Sodium Chloride

Answer: NaCl

Write the formula for Sodium Cyanide

Answer: NaCn

Write the formula for Aluminum Nitrate

Answer: Al(NO3)3

Write the formula for Aluminum Chloride

Answer: AlCl3

Write the formula for Zinc Chloride

Answer: ZnCl2

Write the name for Li2F

Answer: Lithium Fluoride

Write the name for HgO2

Answer: Mercury (II) Oxide

Write the name for HBr

Answer: Hydrobromic Acid

Write the name for CaS

Answer: Calcium Sulfide

Write the name for CCl4

Answer: Carbon Tetrachloride

Write the name for HF

Answer: Hydrofluoric Acid

Write the name for PCl5

Answer: Phosphorous Pentachloride

Write the name for Al2O3

Answer: Aluminum Oxide

Write the name for H2SO4

Answer: Sulfuric Acid

Write the name for Ca3(PO4)2

Answer: Calcium Phosphate

What is the difference between wavelength and frequency?

Answer: Wave,entry differs from frequency because with a longer wavelength the lower the frequency and vice versa.

Electron Configuration for Fe

Answer: [Ar] 4s2 3d6

Electron Configuration for Sc

Answer: [Ar] 4s2 3d1

Which of the following properties generally decreases across the periodic table from sodium(Na) to Chlorine (Cl)?

Answer: Atomic Radius

The fourth principle energy level has:

Answer: Sixteen (16) Orbitals

As the wavelength of light decreases, the energy:

Answer: Increases

Which have the same outer energy level configurations?

1) H, He
2) N, P, As, Bi
3) Mg, Al, Ca, Ga
4) Li, Be, N, Ne

Answer: 2) N, P, As, Bi

The distance between two successive peaks or troughs in a wave is called

Answer: The wavelength

The correct electron configuration for Cu is:

Answer: [Ar] 4s1 3d10

A packet of energy of electromagnetic radiation is called

Answer: Photon

The lowest possible energy state of an atom is called its ___________ state.

Answer: Ground

The energy levels of the hydrogen atom (and all atoms) are _____________, meaning that only certain discrete energy levels are allowed.

Answer: Quantized

According to the VSEPR model, the progressive decrease in the bond angles in the series of molecules CH4, NH3, and H2O is best accounted for by the

Answer: Increasing number of unshared pairs of electrons

Which of the following is an incorrect designation for an atomic orbital?

1) 1s
2) 3d
3) 6s
4) 4f
5) 1p

Answer: 5) 1p

Which of the following elements needs three electrons to complete its valence shell?

1) Ba
2)P
3) Si
4) Ca
5) Cl

Answer: 2) P

The maximum number of electrons in the third principal energy level of an atoms is

Answer: 18

Which one of the following atoms has a partly filled D-Sublevel?

1) Ca
2) Ar
3) Zn
4) As
5) Ni

Answer: 5) Ni

Which of the following atoms has the largest atomic radius?

1) Na
2) Si
3) Mg
4) C
5) P

Answer: 1) Na

Which of the following atoms has the highest ionization energy?

1) P
2) Mg
3) Si
4) Na
5) Cl

Answer: 5) Cl

Which statement is incorrect about quantum theory?

1) when filling orbitals of equal energy two electrons will occupy the same orbital before filling
2) Trick question
3) no electrons can have the same four quantum numbers

Answer: 1) when filling the orbitals of equal energy, two electrons will occupy the same orbital before filling a new orbital

Which molecule has trivial pyramidal geometry?

1) Co2
2) PH3
3) CH4
4) C2H4
5) H2O

Answer: 2) PH3

Which molecule has a double bond?

1) Co2
2) PH3
3) CH4
4) C2H4
5) H2O

Answer: 5) H2O

How many electrons are lost or gained to form the following ions? Al 3+

Answer: Lose 3 electrons

How many electrons are lost or gained to form the following ions? P 3-

Answer: Gain 3 electrons

How many electrons are lost or gained to form the following ions? Pb 2+

Answer: Lose 2 Electrons

How many protons and electrons? Cl -1

Answer: P= 17. E= 18

How many protons and electrons? Al 3+

Answer: P= 13. E= 10

How many protons and electrons? P 3-

Answer: P=15. E=18

How many protons and electrons? Co 2+

Answer: P= 27. E=25

Name two elements that have similar properties similar to those of the element chlorine.

Answer: Iodine and Fluorine (I & F)

How many sig figs? 3670.03

Answer: 6

How many sig figs? 78.65

Answer: 4

How many sig figs? 78.00

Answer: 4

How many sig figs? 9400

Answer: 2

How many sig figs? 0.056

Answer: 2

How many sig figs? 0.0008

Answer: 1

How many sig figs? 406

Answer: 3

How many sig figs? 546.8

Answer: 4

How many sig figs? 4760

Answer: 3

How many sig figs? 6700.3

Answer: 5

The alkaline earth metal that has 18 electrons as a stable ion

Answer: Ca

The halogen that is also a metalloid

Answer: At

The transition metal that has 24 electrons as a 3+ ion

Answer: Co

The heaviest naturally occurring noble gas

Answer: Rn

The atomic mass of an element is equal to______

Answer: The total mass of the isotopes of that element

Which of the following does not belong to the family or classification indicated?

1) Ge, transition metal
2) At, halogen
3) Rn, noble gas
4) Na, alkali metal
5) Eu, lanthanides metal

Answer: 1) Ge, transition metal

A species with 12 protons and 10 electrons is

Answer: Mg 2+

All of the following are characteristics of metals except:

1) conductors of electricity
2) malleable (easy to bend)
3) ductile (can handle impact)
4) often lustrous (shiny)
5) tend to gain electrons in chemical reactions

Answer: 5)tend to gain electrons in chemical reactions

An isotope, X, of a particular element has an atomic number of 7 and a mass of 15 therefore:

X is an isotope of nitrogen
X has 8 neutrons per atom

Answer: X has an atomic number of 14.0067

Which one of the following statements about structure is false?

1) Electrons occupy a very large volume compared to the nucleus
2) Number of protons and neutrons is always the same in the neutral atom
3) protons and neutrons in the nucleus are tightly packed

Answer: (2) number of protons and neutrons is always the same in neutral atom

Which pair has approximately the same mass?

A) a hydrogen, H-1, atom, and a deuterium, H-2 atom
B) a proton and a neutron

Answer: B) a proton and a neutron

Which is false:

1) ions are formed by adding electrons to a neutral atom
2) ions are formed by changing the number of protons in an atoms nucleus
3) ions are formed by removing electrons from a neutral atom
4) an ion has a positive or negative charge
5) metals tend to form positive ions

Answer: (2) ions are formed by changing the number of protons in an atoms nucleus

Which atomic particle determines the chemical behavior of an atom?

Answer: Nucleus

How many protons, electrons, and neutrons does 32 S 16 have?

Answer: 16 Protons 16 Electrons 16 Neutrons

Which statements are true:

1) Number of protons in an element is the same for all neutral atoms of that element
2) The number of electrons in an element is the same for all neutral atoms of that element.
3) The number of neutrons in an element is the same for all neutral atoms of that element.

Answer: None of Them

The average mass of boron is 10.81g. Assuming you were able to isolate one boron atom, the chance that you would randomly get one with a mass of 10.81 is:

Answer: Greater than 50%

Rutherford experiment was important because it showed that:

Answer: An atom is mostly empty space

If E is the symbol for an element, which two of the following represent isotopes of the same element

1) 20 E 10
2) 21 E 9.
3) 20 E 11.
4) 21 E 10

Answer: 1 & 4

How many significant figures are there in the number 0.04560700?

A) 7
B) 5
C) 9
D) 8
E) 4

Answer: A) 7

1a & 1b The product of 0.1400 x (6.02x10 to the 23rd) will have how many signifigant figures (sig figs)

Answer: 3

1a & 1b Express 30,502,000 in scientific notation.

Answer: 3.0502 x 10 to the 7th

The cation Fe3+ is formed when

A) an atom of iron loses two electrons
B) an atom of zinc loses two electrons
C) an atom of iron loses three electrons
D) an atom of iron gains three electrons

Answer: C) an atom of iron loses three electrons

A cation is any atom or group of atoms with

A) a positive charge
B) no charge
C) a negative charge
D) more electrons that the corresponding atoms

Answer: A) A positive Charge

Which element when combined with chlorine would most likely form an ionic compound?

A) lithium
B) carbon
C) phosphorus
D) bromine

Answer: A) Lithium

Which of these is not a characteristic of most ionic compounds?

A) solid at room temperature
B) has a low melting point
C) conducts an electric current when melted
D) produced by reaction between metallic and nonmetallic elements

Answer: B) Has a low melting point

An ionic compound is

A) electrically neutral
B) held together by ionic bonds
C) composed of anions and cations
D) all of the above

Answer: D) All of the above

In forming chemical bonds, atoms tend to attain

A) A state of higher energy
B) the electron configuration of noble gas atoms
C) the electron configuration of halogen atoms
D) all of the above

Answer: B) The electron of noble gas atoms

When an aluminum atom loses its valence electrons, what is the charge on the resulting ion?

A) 2+
B) 2-
C) 3+
D) 1+

Answer: C) 3+

How many valence electrons does an atom of any element in group 6A have?

A) 2
B) 4
C) 6
D) 8

Answer: C) 6

How much energy (in kJ) do 3.0 moles of photons all with a wavelength of 655 nm, contain?

How many photons are contained in a flash of green light (525 nm) that contains 189 kJ of energy?

How many photons are contained in a burst of yellow light (589 nm) from a sodium lamp that contains 609 kJ of energy?

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.

Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm.

Which of the following occur as the wavelength of a photon increases?

Which of the following occur as the energy of a photon increases?

Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 486.1 nm.

Calculate the energy of the orange light emitted per photon, by a neon sign with a frequency of 4.89 × 1014 Hz.

Calculate the energy of the green light emitted per photon, by a mercury lamp with a frequency of 5.49 × 1014 Hz.

Calculate the frequency of the red light emitted by a neon sign with a wavelength of659.9 nm.

Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz.

Calculate the wavelength (in nm) of a the red light emitted by a neon sign with a frequency of 4.74 × 1014 Hz.

Which of the following types of electromagnetic radiation has the smallest frequency?

Which of the following types of electromagnetic radiation has the shortest wavelength?

Which of the following visible colors of light has the longest wavelength?

Which of the following visible colors of light has the largest frequency?

Identify the color that has a wavelength of 460 nm.

Identify the color that has a wavelength of 700 nm.

Place the following types of electromagnetic radiation in order of decreasing energy.ultraviolet light radio waves microwaves

Place the following types of electromagnetic radiation in order of increasing frequency.visible light microwaves X-rays

Place the following types of electromagnetic radiation in order of increasing wavelength.ultraviolet light gamma rays radio waves

A hydrogen atom absorbs a photon of UV light and its electrons enter the n =4 energy level. Calculate the change in energy of the atom and the wavelength (in nm) of the photon.

Green light has a wavelength of 5200 A. Calculate the energy of one photon of green light.

Infrared radiation from the the sun has a wavelength of 6200 nm. Calculate the energy of one photon of that radiation?

A radio has a frequency of 8.6 X 10^8 Hz. What is the energy of one photon of this radiation?

A cook uses a microwave oven to heat a meal. The wavelength of the radiation is 1.20 cm. What is the energy of one photon of this microwave oven?

Yellow light has a frequency of 5.2 x 1014 s -1 while red light has a frequency of 4.3 x 1014 s -1 . Which of the following correctly describes the relationship between the wavelength and energy of yellow versus red light?

The energy of the electron of a hydrogen atom in the ground (n = 1) state is ___________.

What is the wavelength of a neutron (the mass of a neutron is 1.675 × 10-27 kg) traveling at 100.0 m/s?

Which equation represents the electron affinity (E.A.) of the tungsten (W, 74) atom?

Given the information below, what is the average valence electron energy for the oxygen atom (O, 8)? Ionization Energies (in unites of MJ/mol) Element 1s 2s 2p O 52.6 3.12 1.31

Which of the following atoms or ions is the smallest?

Arrange the following four atoms in order from smallest to largest radius: Fluorine (F, 9); Neon (Ne, 10); Sodium (Na, 11); Magnesium (Mg, 12)

Which of the following atoms contains the most unpaired electrons in its ground state?

Which electron configuration of p orbitals would satisfy Hund's rules?

What -2 ion can have an electron configuration of 1s2 2s2 2s6 3s1 3p1 ?

What is the correct electron configuration for the zirconium (Zr, 40) atom?

A possible set of quantum numbers for the last electron added to form a gallium atom (Ga, 31) in its lowest energy state is:

The Pauli exclusion principle states that:

In a single atom, what is the maximum number of electrons could have a principal quantum number (n) of 4 and an angular quantum number (l) of 1?

Which of the following quantum numbers is used to describe the orientation of an orbital in space?

Which of the following elements requires the most energy to remove its most tightly held electron (the electron closest to the nucleus): Magnesium (Mg, 12); Aluminum (Al, 13); Silicon (Si, 14); Phosphorus (P, 15); Sulfur (S, 16)

Which element is represented by the following PES spectrum?

An atom in its ground state absorbs two photons: a photon with a wavelength of 102.6 nm and then a photon with a wavelength of 1875 nm. The atom then relaxes back to the ground state by emitting a single photon. What is the wavelength of the emitted photon?

The first ionization energy of the first six elements in the periodic table is given below. H 1312.0 kJ/mol He 2372.3 Li 520.2 Be 899.4 B 800.6 C 1086.4 Why is the first ionization energy of B smaller than Be?

Arrange the following elements in order of increasing first ionization energy: Sulfur (S, 16); Argon (Ar, 18); Calcium (Ca, 20)

Which of the following transitions from a hydrogen atom with an electron in the n = 5 state will result in the emission of the longest wavelength of light?

The line structure of the emission spectrum of the hydrogen atom suggests that:

What is the wavelength, in meters, of light that has a frequency of 2.33 x 1015 s -1 ?

If X-rays have a shorter wavelength than ultraviolet light, which of the following statements is true?

What is the frequency of radiation of wavelength 810 nm?

How many photons are in a 1.20mJ burst of this radiation?

If the 330 nm radiation provides exactly the energy to break an average chemical bond in the skin, estimate the average energy of these bonds in kJ/mol.

One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 330 nm .What is the energy of a photon of this wavelength?

Which of the following statements concerning experiment and explanation is/are true?

Which nuclide has the same number of protons as ¹⁴₇N?

The property of a series of repeated measurements that is most directly related to precision is

An ion is formed

Which of the following conclusion regarding Rutherford's gold foil experiment is not consistent with the observations?

A sample that cannot be separated into two or more substance by physical means is

A sample of silicon is burned in oxygen to form silicon dioxide. What mass of oxygen is consumed if 57.76 g silicon dioxide is formed from 27.00 g silicon?

6.7 kilogram(s) contains this many grams:

How many oxygen atoms are there in a formula unit of UO₂(C₂H₃O₂)₂ • NH₄C₂H₃O₂ • 4H₂O?

Cathode rays are

Neon has three naturally occurring isotopes. The abundance of ²⁰Ne is 90.48% and ²²Ne is 9.25%. What is the percent abundance of ²¹Ne?

According to the law of multiple proportions:

The average speed of oxygen molecules at 690°C is 1.60 × 10⁵ cm/s. Which of the following calculations would convert this speed to units of miles per hour?

Choose the group containing the most reactive nonmetals.

What is the volume of a cube that has an edge length of 0.019 m?

In a particular mass of KAu(CN)₂, there are 8.87×10²⁰ atoms of gold. What is the total number of atoms in this sample?

A species that is formed when a molecule gains or loses an electron is called

Which of the following statement concerning the SI system is/are correct?

A 4.06 cm³ sample sodium metal has a a density of 0.968 g/cm³. What volume does this sample of sodium occupy in its liquid state? The density of liquid sodium is 0.927 g/cm³.

Calculate the frequency of the red light emitted by a neon sign with a wavelength of
659.9 nm.

Place the following types of electromagnetic radiation in order of decreasing energy.
ultraviolet light radio waves microwaves

Place the following types of electromagnetic radiation in order of increasing frequency.
visible light microwaves X-rays

Place the following types of electromagnetic radiation in order of increasing wavelength.
ultraviolet light gamma rays radio waves