A positively charged ion results from _________ electrons.
A. losing
B. gaining
C. sharing
D. destroying
Answer:
A. losing
A positively charged ion results from _________ electrons.
A. losing
B. gaining
C. sharing
D. destroying
Answer:
A. losing
A. losing
B. gaining
C. sharing
D. destroying
Answer:
A. losing
A _______ is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.
A _______ is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.
A. chemical bond
B. electrostatic bond
C. physical bond
D. bonding arrangement
Answer: A. chemical bond
When two or more valid Lewis structures can be drawn for a molecule we get what is called __________.
When two or more valid Lewis structures can be drawn for a molecule we get what is called __________.
A. confused
B. covalent
C. balanced
D. resonance
Answer: D. resonance
Hydrogen bonding can occur when hydrogen is covalently bonded to a highly ___________ atom.
Hydrogen bonding can occur when hydrogen is covalently bonded to a highly ___________ atom.
A. electronegative
B. stable
C. ionized
D. unstable
Answer: A. electronegative
London dispersion forces are the result of the movement of __________.
London dispersion forces are the result of the movement of __________.
A. protons
B. neutrons
C. electrons
D. ions
Answer: C. electrons
When one atom has a higher electronegativity than the other a __________ covalent bond will result.
When one atom has a higher electronegativity than the other a __________ covalent bond will result.
A. polar
B. metallic
C. nonpolar
D. dipole
Answer: A. polar
Electrons are shared equally in ________ covalent bonds.
Electrons are shared equally in ________ covalent bonds.
A. polar
B. metallic
C. nonpolar
D. dipole
Answer: C. nonpolar
A charged group of covalently bonded atoms is called a ___________.
A charged group of covalently bonded atoms is called a ___________.
A. polyatomic ion
B. ionic covalent molecule
C. polar ion
D. alloy
Answer: A. polyatomic ion
A ___________ is created by equal but opposite charges that are separated by short distance.
A ___________ is created by equal but opposite charges that are separated by short distance.
A. dipole
B. coordinate
C. longitudinal force
D. polar force
Answer: A. dipole
A __________ is a neutral group of atoms held together by covalent bonds.
A __________ is a neutral group of atoms held together by covalent bonds.
A. mixture
B. ion
C. alloy
D. molecule
Answer: D. molecule
A _________ bond joins atoms together by sharing electrons.
A _________ bond joins atoms together by sharing electrons.
A. ionic
B. metallic
C. covalent
D. mixture
Answer: C. covalent
The strength of metallic bonds is given by ____________.
The strength of metallic bonds is given by ____________.
A. bond breaking energy
B. bond dissociation energy
C. covalent energy
D. enthalpy of vaporization
Answer: D. enthalpy of vaporization
Valence electrons in metal atoms can be modeled as
Valence electrons in metal atoms can be modeled as
A. a sea of electrons
B. columns of electrons
c. a kiddy pool of electrons
D. various groups of electrons
Answer: A. a sea of electrons
Ionic compounds are electrically
Ionic compounds are electrically
A. positive
B. neutral
C. negative
D. either positive or negative
Answer: B. neutral
Whether a bond will be ionic or covalent depends on the difference in __________ of the atoms involved.
Whether a bond will be ionic or covalent depends on the difference in __________ of the atoms involved.
A. Ionization energy
B. electronegativity
C. number of valence electrons
D. atomic radius
Answer: B. electronegativity
Negatively charged ions are called
Negatively charged ions are called
A. cations
B. anions
C. negions
D. minusions
Answer: B. anions
Explain why hydrogen bonds are stronger than most dipole-dipole forces.
Explain why hydrogen bonds are stronger than most dipole-dipole forces.
Answer: A hydrogen bond involves a large difference in electronegativity between the hydrogen atom and the atom it is attached to (O, N or F), making the bond extremely polar.
Why are dispersion forces weaker than dipole-dipole forces?
Why are dispersion forces weaker than dipole-dipole forces?
Answer: Dispersion forces are between temporary dipoles (nonpolar molecules). dipole-dipole forces are between permanent dipoles (polar molecules).
Explain the difference between a temporary dipole and a permanent dipole.
Explain the difference between a temporary dipole and a permanent dipole.
Answer: A temporary dipole forms when one molecule is close to another molecule and the electrons repel each other creating a greater electron density in one part of the molecule. permanent dipoles are found in polar molecules in which some regions of the molecule are always partially positive and partially negative.
Compare the location of bonding electrons in a polar covalent bond with those in a nonpolar covalent bond.
Compare the location of bonding electrons in a polar covalent bond with those in a nonpolar covalent bond.
Answer: electrons in a polar bond are closer to the more electronegative atom because of unequal sharing. those in a non polar bond are equally shared.
Explain the difference between non polar molecules and polar molecules.
Explain the difference between non polar molecules and polar molecules.
Answer: a nonpolar molecule has a symmetric distribution of charge while a polar molecule has concentration of electrons on one side of the molecule.
Describe electronegativity trends in the periodic table.
Describe electronegativity trends in the periodic table.
Answer: it increases left to right in a period and decreases top to bottom in a group.
What must you know in order to draw the Lewis structure for a molecule?
What must you know in order to draw the Lewis structure for a molecule?
Answer: The number valence electrons each atom contributes to the molecule.
Explain the difference between sulfur hexafluoride and disulfur tetrafluoride.
Explain the difference between sulfur hexafluoride and disulfur tetrafluoride.
Answer: sulfur hexafluoride has one sulfur bonded to 6 fluorines. disulfur tetrafluoride has 2 sulfur atoms bonded to 4 fluorine atoms.
Explain how molecular compounds are named.
Explain how molecular compounds are named.
Answer: Prefixes used to show how many of each atom are in the molecule, ending of second element changed to -ide.
Describe the forces, both attractive and repulsive, that occur as two atoms move closer together.
Describe the forces, both attractive and repulsive, that occur as two atoms move closer together.
Answer: as the atoms approach, the net force of attraction increases. at a certain optimal distance between atoms, the net attractive force is maximized. if the atoms move closer than the optimal distance, repulsive force exceeds attractive force.
Describe the bonding in molecules.
Describe the bonding in molecules.
Answer: atoms share electrons within a molecule, creating covalent bonds.
Describe the formation of a covalent bond.
Describe the formation of a covalent bond.
Answer: The nucleus of an atom attracts the electrons of another atom and they share one or more electron pairs.
What is the octet rule, and how is it used in covalent bonding?
What is the octet rule, and how is it used in covalent bonding?
Answer: Atoms will share electrons (bond) to achieve a full valence shell with 8 electrons in it.
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