NAME___________________________
Planck’s constant: 6.626 x 10-34 j-s
Mass of proton: 1.67262 x 10-27kg
10/18 ws ch 7, part of 8 Exam Tues. 10/22
speed of light: 2.9979 x 10 8 m/s
R = 2.178 x 10-18 j
mass of neutron: 1.67493 x 10 -27kg mass of e- = 9.10930 x 10-31 kg Avo #: 6.022 x 1023
1] If the frequency of light is 6.12 x 10 15 Hz, find the wavelength in angstroms, and determine if the light is uv, ir, or visible.
2] If the frequency of light is 7.4 x 1014Hz, what is the energy of this light per photon, and in one mole of photons?
3] A radio station broadcasts at 1280 kHz. Find its wavelength.
4] If the bond strength of a C – C bond is 347 kj/mol, what is the maximum wavelength of light, in A o, that could break this bond?
5] If an electron in a hydrogen atom drops from the sixth to the third energy level, find
a] the energy per photon of light that is emitted
b] the frequency of the light c] wavelength, in A o
d] if the light is visible, uv, or ir.
6] Calculate the wavelength of an electron moving at 0.010% of the speed of light.
7] Find x for a 125 g ball if v is 0.100 m/s.
8] Find x for an electron if v is 0.100 m/s.
9] Define/explain:
a] wavelength
h] valence electron
b] frequency
I] alkali metal
c] photon
j] alkali-earth metal
d] ground state
k] halogen
e] excited state
l] ionization energy
f] orbital
m] electron affi nity
g] 2 (psi squared)
n] electronegativity
o] ionic bond
u] isoelectronic
p] covalent bond
v] polar covalent bond
r] dipole
w] photoelectric effect (picture)
s] diffraction (picture)
x] Heisenberg uncertainty principle
t] Hund’s rule
y] metalloid
10] Why do successive ionization energies always increase?
11] How do 3d and a 4d orbitals differ from one another?
12] Write the expected electron configuration for:
+
11Na
a] 4Be
b] 81Tl
c]
d] 43Tc
e] 68Er
f] 34Se-2
13] Find the number of unpaired electrons for the element/ions in #12.
A]
b]
c]
d]
e]
f]
14] What neutral, ground state element has its highest energy electron described by the quantum numbers:
a] n = 5;
l = 0;
ml = 0; ms = +1/2
b] n = 4;
l = 1;
ml = +1; ms = -1/2
c] n = 3;
l = 2;
ml = -2; ms = -1/2
d] n = 5;
l = 3;
ml = +1; ms = +1/2
e] n = 2;
l = 2;
ml = 0; ms = +1/2
f] n = 5;
l = 1;
ml = -2; ms = -1/2
15] Put in order from lowest to highest atomic radius:
a] Ga, P, As
b] Mg, Mg+1, Mg+2
c] Mg+2, Ne, O-2, Na+
16] Put in order of increasing ionization energy:
a] P, Si, N
b] C, P, As
c] Mg, Mg +1, Mg+2
17] Elements Q, R, T and M have electronegativities of 1.0, 1.7, 2.7 and 3.5 respectively. For the bonds below, identify
the bond type (ionic, covalent, polar covalent, pure covalent), the direction of polarity, and list the bonds from least to
most polar.
M–M
Q–T
Q–M
M–T