Atoms n' Ions (Equations too)
Aqueous Solutions and Thermochemistry
Electronic Structure and Periodic Trends
Chemical Bonding and Molecular Geometry
Random Calculations
100
What is the name of the outermost electrons?
Valence electrons
100
What are the 5 kinds of reactions you typically see in class/textbook?
Combination, Decomposition, Single Replacement, Double Replacement, Combustion
100
Using
∆E = (-2.18 x 10-18 J) ((1/nf2) - (1/ni2)),
how much energy was released when an electron jumps to n=1 from n=3?
-1.94 x 10-18 J
100
What hybridization does this molecule have?
H - N - H
|
H
sp3
100
What is the formal charge for each atom in the molecule:
CCl2O
C: 0
Cl: 0 for both
O: 0
200
What are the names of the Group 7 and 8 elements?
Halogens and Noble Gases
200
What two anions are always soluble?
NO3- and CH3COO-
200
What is the trend of Z(effective) across a period? Explain
Across a period, Z(eff) increases because the number of protons increases while the number of shielding electrons (Core electrons) remains the same
200
In _________ bond(s), bonding electrons are shared such that all particles, after bonding, have the same number of electrons as a noble gas.
a) Nonpolar covalent bonds
b) Polar covalent bonds
c) Ionic bonds
d) A and B
e) A, B, and C
d) A and B
200
How many grams of K2SO4 are needed to react with 85.3 g of AlBr3?
83.6 g K2SO4
300
Which subatomic particles are the same in a given set of isotopes?
Protons and Electrons
300
Calculate the enthalpy for this reaction:
2C(s) + H2(g) ----> C2H2(g)
Given the following equations:
C2H2(g) + 5/2 O2(g) ---> 2CO2(g) + H2O(l) ΔH°= -1299.5 kJ
C(s) + O2(g) ---> CO2(g) ΔH° = -393.5 kJ
H2(g) + 1/2 O2(g) ---> H2O(l) ΔH° = -285.8 kJ
+226.7 kJ
300
Which term states that when filling orbitals in a subshell, each one should have one electron before adding another with the opposite spin?
Aufbau Principle
Hund's Rule
Pauli-Exclusion Principle
Hund's Rule
300
Find the bond enthalpy of the unbalanced reaction (make sure to balance):
C3H8 + O2 ----> CO2 + H2O
-2060 kJ/mol
300
A balloon inflated with three breaths of air has a volume of 1.92 L. At the same temperature and pressure, what is the volume of the balloon if five more same-sized breaths are added to the balloon?
5.12 L
400
In the combustion of 67.32g of butane (C4H6), how many grams of CO2 are produced?
Write and balance the equation before solving
203.8 g CO2
400
A 23.6 g sample of Ethanol releases 4151 J as it cools from 95.8 oC. Calculate the final temperature of the ethanol.
Use 2.46 J/g C for specific heat of Ethanol
24.3 oC
400
What is the electron configuration of Cr+3?
1s22s22p63s23d3
400
What is the electron (domain) geometry, molecular geometry, and hybridization of the central atom for the ICl4- ion?
Electron geometry: Octahedral
Molecular geometry: Square Planar
Hybridization: sp3d2
400
Find the heat of formation for a mole of carbon monoxide given:
CO2(g) + C(s) ----> 2CO(g) ∆H = 172.5 kJ
C(s) + O2(g) ----> CO2(g) ∆H = -393.5 kJ
Use kJ and 3 sig figs in your final answer
C(s) + 1/2 O2(g) ----> CO(g)
∆Hof = -1.10 x 102 kJ
500
Balance the equation:
S + HNO3 ----> H2SO4 + NO2 + H2O
S + 6 HNO3 ----> H2SO4 + 6 NO2 + 2 H2O
500
What is the concentration of Sr(OH)2 if a 2 L solution of containing 45.3 g of HCl was used, and only 65.9 mL of HCl was needed to neutralize 12.4 mL of Sr(OH)2?
1.65 Molar Sr(OH)2
500
What is the energy of a photon with a wavelength of 325 nm? What about the energy of one mole of these photons?
First answer should have the unit J/photon
Second answer should have the unit kJ/mol
6.11 x 10-19 J/photon
368 kJ/mol
500
Draw the lewis dot structure for H2SO4 (H is bonded to O)
500
If a square piece of gold foil contains about 1.73 x 1022 atoms of Au and the thickness is 0.0000173 cm, what is the length of one side of the foil?
Density of gold: 19.3 g/mL
1.30 x 102 cm