Chapter 5-8

Chapter 5

100

Calculate Delta E and determine whether the process is endothermic or exothermic if q = 0.763 kJ and w = -840 J

delta E= -0.077kJ, endothermic

200

Ozone (O₃) decomposes to O₂ gas at room temperature and pressure according to the following reaction:

2O₃(g) -> 3O₂(g)  delta H=-284.6kJ

Which has the higher enthalpy under these conditions, 2O₃(g) or 3O₂(g) ?

2O₃(g) has the higher enthalpy

300

Calculate the enthalpy change for the reaction

P4O₆(s) + 2O₂(g) -> P₄O₁₀(s)

given the following enthalpies of reaction

P₄(s) + 3O₂(g) -> P₄O₆(s) delta H= -1640.1kJ
P₄(s) + 5O₂(g) -> P₄O₁₀(s) delta H= -2940.1kJ

delta H = -1300.0kJ

400

Given the solution

Ag⁺(aq) + Cl^-(aq) -> AgCl(s) delta H= -65.5kJ

calculate delta H for the production of 0.450 mol of AgCl

-29.5kJ mol/delta H

500

Using the given values, calculate the standard enthalpy change for the following reaction:

SiCl₄(l) + 2H₂O(l) -> SiO₂(s) + 4HCl(g)

SiCl₄(l) = -640.1kJ/mol
H₂O(l) = -285.8kJ/mol
SiO2(s) = -910.9kJ/mol
HCl(g) = -92.3kJ/mol

delta H_rxn = -68.3kJ

Chapter 6

100

A laser pointer emits light at 650 nm. What is the frequency of this radiation? What color is associated with this wavelength?

4.61x10¹⁴ s^-1

red

200

What is Heisenberg's uncertainty principle?

The position and velocity of an electron cannot be found at the same time; you can't know both

300

If n=4, what are the possible values of l?

l = 3,2,1,0

400

Is energy emitted or absorbed when the following electronic transitions occur in hydrogen? from n = 4 to n = 2

emitted

500

Arrange the kinds of electromagnetic radiation in order of increasing wavelength: infrared, ultraviolet light, green light, X rays, red light, radio waves

Xray < ultraviolet < green light < red light < infrared light < radio waves

Chapter 7

100

Arrange the set of atoms in order from largest to smallest:

F, O, N

N > O > F

200

Based on their positions in the periodic table, predict which of the following atoms will have a smaller first ionization energy

K, Co

K

300

Which has a larger atomic radius and why?

S^2- and O^2-

S^2- because the size of an atom increases going down a family

400

Predict whether the following oxide is ionic or molecular:

Al₂O₃

Ionic

500

Write a balanced equation for the following reaction:

Strontium oxide is added to water

SrO(s) + H₂O(l) -> Sr(OH)₂(aq)

Chapter 8

100

Is this bond polar or nonpolar?

Se-O

Polar

200

Which of the following statements about formal charge is true?

1. Formal charge is the same as oxidation number
2. To draw the best Lewis structure, you should minimize formal charge
3. Formal charge takes into account the difference electronegativities of the atoms in a molecule
4. Formal charge is most useful for ionic compounds
5. Formal charge is used in calculating the dipole moment of a diatomic molecule

2

300

Draw the resonance structure for the nitrite ion

Nitrogen single bonded to 1 Oxygen with a minus 1 formal charge and double bonded to 1 Oxygen

400

Estimate delta H for the following reaction

H₂(g) + Br₂(l) -> 2 HBr(g)

Using the following bond enthalpy values:

H-H 436 kJ/mol
H-Br 366 kJ/mol
Br-Br 193 kJ/mol

delta H =-103 kJ/mol

500

What is the noble gas electron configuration for Cr

[Ar]4s¹3d⁵

Mystery 3x points

100

How many unpaired electrons are there in Mn

5

200

What does a double bond consist of?

one sigma and one pi bond

300

In ionic bond formation, the lattice energy of ions ____ as the magnitude of the ion charges _____ and the radii ______

increases, increase, decrease

400

PCl₅ has _____ electron domains and a _____ molecular arrangement

5; trigonal bipyramidal

500

What is the binding energy of an electron in a photosensitive metal (in kJ/mol) if the minimum frequency of light that can eject protons from the metal is 6.85x10¹⁴ Hz

273.3 kJ/mol