I. The number of protons in an element is the same for all neutral atoms of that element.
II. The number of electrons in an element is the same for all neutral atoms of that element.
III. The number of neutrons in an element is the same for all neutral atoms of that element
a. two atoms of gallium and three atoms of oxygen
b. six atoms of each element
c. three atoms of gallium and two atoms of oxygen
d. five atoms of each element
e. none of the above
In the following list, only _______ is not an example of a chemical reaction.
A) Dissolution of a penny in nitric acid
B) the condensation of water vapor
C) a burning candle
D) the formation of polyethylene from ethylene
E) the tarnishing of silver
The following combinations of quantum numbers are not allowed. Correct each set by changing only one quantum number, and write in an appropriate corrected value.
a. n = 2 l = 2 ml = 2 Corrected: _____ = _____
b. n = 4 l = -2 ml = 0 Corrected: _____ = _____
What is the difference between a theory and a law? What is the collision theory?
Answer: a law is a statement of what will happen while a theory explains why something happens. the collision theory states that atoms, ions, and molecule can react to form products when they collide
Explain the context and meanings of the terms "orbit" and "orbital", making a clear distinction between them.
Answer: Orbit is a term from the Bohr theory, and refers to an exact, circular path followed
by an electron. It has been superseded by the concept of an orbital, which arises from the Schrodinger equation. An orbital is a wave function, or, more loosely, a region of space close to the nucleus where an electron is likely to be found.
In the quantum mechanical treatment of the hydrogen atom, the functions and 2 both feature prominently. Briefly explain (in principle) how they are obtained and what, if anything, their physical meanings are.
Solution: The wave function, is a solution to the Schrodinger equation. It describes a wave, but has no physical meaning of its own. The square of the wave function, 2, represents the probability of finding the electron at any point in the atom.
Would the photon in (a) have enough energy to ionize a hydrogen atom in its ground state (i.e., to separate the proton and electron completely)? Use the Bohr equation to explain your answer.
Answer: No. 2.18 x 10^-18 J is needed, the difference between the n = 1 and n = infinity levels.
Use the Rydberg equation to calculate the wavelength, in nm, of the least energetic (longest wavelength) line in the visible series (n1 = 2) of the spectrum of atomic hydrogen.