Precipitation and Molarity
Oxidation and Reduction
Wavelength and Frequency
Quantum Numbers
Miscellaneous
100

Difference between total ionic and net ionic equation

A net ionic equation shows only the elements and compounds that are involved in a

reaction, while a complete ionic equation also includes the spectator ions

100

Define oxidation and reduction

Oxidation is the loss of electrons and Reduction is the gain of electrons

100

Calculate the frequency of blue light having a wavelength of 350 cm

8.57 x 107 Hz

100

How many nodes are in P, S, F, and D orbital

P = 2, S = 1, F = 8, D = 4

100

Write the condensed electron configuration for Cu

[Ar]4s13d10

200

Does a precipitate form for this chemical equation: AgNO3(aq) + KCl(aq) →

Answer: Yes

AgCl(s) + KNO3(aq)

200

MnO2 (Find the oxidation number of Mn)

+4

200

What is the energy of a photon with a wavelength of 200 cm?

9.939 x 10-26 J

200

Determine the sublevels for 3

s, p, d


200

What is the pOH of a 0.0235 M HCl solution?

12.371

300

How many grams of hydrogen chloride (HCl) are required to prepare 500 mL of 5M HCl in water?

91.25 g HCl

300

Determine what is being oxidized and what is being reduced: 2HCl (aq) + Zn (s) → H2 (g) + ZnCl2 (aq)

Oxidized is Zn

Reduced is H in HCl

300

Determine the wavelength of light emitted when an electron of an helium atom makes a transition from orbital 3 to orbital 6

-1.094 x 10-6

300

Given the information find the n, l, and ml: 4d

n=4, l = 2, ml = -2, -1, 0, 1, 2

300

Is there something called a 1d or 2d orbital?

No

400

Using the chemical equation how many grams of HCl is required to neutralize 20.0 mL of 0.5 mol NaOH? HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

0.365 g HCl

400

Balance the chemical equation and determine what is being oxidized and what is being reduced: AlCl3 (aq) + Mg (s) → Al (s) + MgCl2 (aq)

2AlCl3 (aq) + 3Mg (s) → 2Al (s) + 3MgCl2 (aq)

Oxidized is Mg

Reduced is Al in AlCl3

400

When an electron absorbs -4.0 x 10-35 J of energy and ascends from energy level 2, what energy level does the electron end at?

2

400

Write a set of quantum number for 3p

n=3, l = 1, ml = -1, 0, 1

400

Give the definitions for Aufbau principle, Pauli exclusion principle, and Hund's rule

Aufbau Principle: Lower energy orbitals fill first

Pauli Exclusion principle: Degenerate orbitals (those of the same energy) are filled with electrons until all are half-filled before pairing up of electrons

Hund's rule: Individual orbitals only hold two electrons, and each should have a different spin

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