hydrobromic acid

HBr

strong acid

hydroiodic

HI

strong acid

nitric

HNO₃

strong acid

perchloric acid

HClO₄

strong acid

sulfuric acid

H₂SO₄

strong acid

lithium hydroxide

LiOH

strong base

potassium hydroxide

KOH

strong base

sodium hydroxide

NaOH

strong base

barium hydroxide

Ba(OH)₂

strong base

strontium hydroxide

Sr(OH)₂

strong base

ammonia

NH₃

weak base

hydrofluoric acid

HF

weak acid

phosphoric acid

H₃PO₄

weak acid

carbonic acid

H₂CO₃

weak acid

acetic acid

C₂H₄O2

weak acid

precipitation reaction

aqueous sol + aqueous sol = insoluble sol + aqueous sol

Net ionic equation for copper III sulfiate (aq) + sodium carbonate (aq)

Cu²⁺ (aq)+ CO₃ ^2- (aq)= CuCO₃ (s)

What is the net ionic equation for the reaction of aqueous sodium iodide and lead(II) nitrate?

Pb²⁺ (aq)+2I^-(aq)=PbI₂ (s)

oxidation rule 1

Pure elements have an oxidation number of 0 e.g. Na, pa, se, Ag (erement).

oxidation rule 2

if the compund is ionic, the oxidation number is the element's charge

oxidation rule 3

hydrogen oxidation number is 1+

oxidation rule 4

oxygen oxidation number is 2-

oxidation rule 5

sum of oxidation numbers is ALWAYS 0

oxidation rule 6

oxidation number in polyatomic ions is the charge

Oxidation

substances transfer/lose electron(s). The substance is a reducing agent

Reduction

substance accepts electron. The substance is an oxidizing agent

which is the oxidizing reactant?

Cu²⁺+Zn -> Zn²⁺+Cu

Cu²⁺

which is the oxidizing agent?

Fe³⁺+Co=Co²⁺+Fe²⁺

Fe³⁺ is the oxidizing agent

A student weighs out 15.8 g of sodium sulfate and transfers it to a 500- mL volumetric flask, adds enough water to dissolve the solid, and then adds water to the 500. mL mark on the neck of the flask. Calculate the concentration ( in molarity units) of sodium sulfate, the sodium ion, and the sulfate ion in the resulting solution. Molar mass of sodium sulfate= 142.0 g/mol

[Na2SO4]=0.222 M, [Na+]= 0.444 M, [SO4 2-]= 0.222 M

Calculate the mass of potassium nitrate required to prepare 500.
mL of 0.125 M potassium nitrate solution using solid potassium
nitrate, a 500. mL volumetric flask, and de-ionized water. M(potassium nitrate)= 101.1 g/mol

6.32g

In the lab, a student dilutes 21.5 mL of a 10.0 M nitric acid solution to a total volume of 125 mL. What is the concentration of the diluted solution?

[HNO3]= 1.72 M

Calculate pH of an aqueous solution of 4.4x10-2 M HCl

1.36

The pH of orange juice is 3.5. What is H3O+ concentration in
solution?

3.16x10^-4

An aqueous solution of HI is standardized by titration with a 0.131 M solution of KOH. If 20.3 mL of base are required to neutralize 26.1 mL of the acid, what is the molarity of the HI solution?

0.102

Calculate the volume of 0.106 M barium hydroxide required to neutralize 18.6 mL of a 0.288 M hydrochloric acid solution

25.3

Your favorite music station is at 99.1 MHz. What is the wavelength of your favorite station? c= 2.998x108 m/s

3.03

Emission

going from a higher energy state to a lower energy state

Energy is emitted

Absorption

going from a lower energy state to a higher energy state

Energy is absorbed

what does a Long wavelength entail?

Long wavelength = low frequency = low energy transition = short line on the diagram

What does a Short wavelength entail?

Short wavelength = high frequency = high energy transition = long line on the diagram

ionization energy

energy required to remove an electron in the ground state (n=1) entirely from the nucleus (n = infinity), leaving H⁺ + e ^-

In the reaction below, the oxidation state of nitrogen changes from ____ to ____.

2 NO(g) + 3 PbO2(s) + 3 SO42–(aq) + 4 H+(aq) 2 NO3–(aq) + 3 PbSO4(s) + 2 H2O(l)

+2, +5

isoelectronic

having the same number of electrons

Which of the following are isoelectronic with Cl^-?

1. Ca²⁺
2. S^2-
3. O^2-

Ca²⁺ and O^2-

If an aqueous solution of ____ is added to a mixture of Cl ^– and SO₄ ^2–, the sulfate ion will precipitate, but the chloride ion will remain in solution.

Ca(NO₃)₂

How many electrons can be described by the following quantum numbers: n = 2, = 1, = –1, m_s = –1/2?

1

Hund's Rule

one electron will occupy each orbital with the same spin before electrons pair in the same orbital

Aufbau Principle

lower energy orbitals should be completely filled before moving on to higher energy orbitals

Pauli Principle

no more than two electrons can occupy one orbital, and if there are two electrons in an orbital they must have opposite spins

How many orbitals have the following set of quantum numbers: n = 5, = 3, = +2?

1

If 83.2 mL of 2.79 M HCl(aq) is diluted with water to a volume of 838 mL, what is the molarity of the diluted HCl(aq)?

0.277M

If 6.90 g NaNO₃ is dissolved in enough water to make 542 mL of solution, what is the molarity of the sodium nitrate solution?

0.150 M

What is the pH of 7.50E-2 M HCl(aq)?What is the pH of 7.50E-2 M HCl(aq)?

1.12

For a hydrogen atom, calculate the wavelength of an emitted photon in the Lyman series that results from the transition n = 2.00 to n = 1.00. Rydberg constant is 1.097E+7 m^–1.
(h = 6.626E-34 J×s and c = 2.998E+8 m/s)

122nm

m to nm

10^9

A mass of 0.3573 g of an unknown acid, HA, is titrated with NaOH. If the acid reacts with 29.05 mL of 0.1149 M NaOH(aq), what is the molar mass of the acid?

107 g/mol

What is the ground state electron configuration for Cr²⁺?

[Ar] 3d⁴

Which of the following atoms is diamagnetic in the ground electronic state?

I

Mn

S

Ge

Sr

Sr

Put the following forms of electromagnetic radiation in order of DECREASING wavelength (longest to shortest):

ultraviolet radiation, infrared radiation, yellow light, blue light

infrared > yellow > blue > ultraviolet

electromagnetic spectrum order

low wavelength to high wavelength

gamma, xray, ultraviolet, visible, infrared, micro, radio

What are the spectator ions in the reaction between aqueous nitric acid and ammonia?

NO₃ ^– only

Which species is reduced in the reaction below?

I^–(aq) + ClO^–(aq) → IO^–(aq) + Cl^–(aq)

ClO^-

Whats the relationship between long lines on the emission/absorption diagrams to

energy, frequency, wavelength

long line: more energy, high frequency, low wavelength

Whats the relationship between short lines on the emission/absorption diagrams to

energy, frequency, wavelength

short line: less energy, less frequency, high wavelength

When going down the groups, what happens to atomic size?

atoms get bigger

When going across (L to R) the periods, what happens to atomic size?

atoms get smaller

What is the net ionic equation for the reaction of aqueous sodium hydroxide and aqueous iron(II) chloride?

Fe²⁺(aq) + 2 OH^–(aq) → Fe(OH)₂(s)

Which of the following sets of quantum numbers are NOT allowed?

1-n = 3, l = 1, m_l = ?1, m_s = +1/2
2-n = 3, l = 2, m_l = ?3, m_s = +1/2
3-n = 4, l = -1, m_l = ?1, m_s = +1/2
4-n = 4, l = 2, m_l = ?2, m_s = +1/2
5-n = 4, l = 1, m_l = ?2, m_s = +1/2

2,3,5

A laser pointer emits light at 646 nm. What is the frequency of this radiation?

4.64E+14 s^-1

Which of the following properties is associated with the value of the quantum number?

shape of orbital

What type of orbital is designated n = 3, = 0, = 0?

3s

What are the spectator ions in the reaction between aqueous ZnCl₂ and aqueous K₂CO₃?

K⁺ Cl^-

What are the oxidation numbers of each manganese in MnO₂ and MnO₄ ^-, respectively?

+4, +7