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1

Electrolyte

Electrolyte is the compound whose aqueous solution conduct electricity

2

Soluble ionic compounds

give off electricity

3

soluble covalent compounds

do not give off electricity

4

hydrochloric acid

HCl

strong acid

5

hydrobromic acid

HBr

strong acid

6

hydroiodic

HI

strong acid

7

nitric

HNO3

strong acid

8

perchloric acid

HClO4

strong acid

9

sulfuric acid

H2SO4

strong acid

10

lithium hydroxide

LiOH

strong base

11

potassium hydroxide

KOH

strong base

12

sodium hydroxide

NaOH

strong base

13

barium hydroxide

Ba(OH)2

strong base

14

strontium hydroxide

Sr(OH)2

strong base

15

ammonia

NH3

weak base

16

hydrofluoric acid

HF

weak acid

17

phosphoric acid

H3PO4

weak acid

18

carbonic acid

H2CO3

weak acid

19

acetic acid

C2H4O2

weak acid

20

precipitation reaction

aqueous sol + aqueous sol = insoluble sol + aqueous sol

21

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

Cu2+ (aq)+ CO3 2- (aq)= CuCO3 (s)

22

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

Pb2+ (aq)+2I-(aq)=PbI2 (s)

23

oxidation rule 1

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

24

oxidation rule 2

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

25

oxidation rule 3

hydrogen oxidation number is 1+

26

oxidation rule 4

oxygen oxidation number is 2-

27

oxidation rule 5

sum of oxidation numbers is ALWAYS 0

28

oxidation rule 6

oxidation number in polyatomic ions is the charge

29

Oxidation

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

30

Reduction

substance accepts electron. The substance is an oxidizing agent

31

which is the oxidizing reactant?

Cu2++Zn -> Zn2++Cu

Cu2+

32

which is the oxidizing agent?

Fe3++Co=Co2++Fe2+

Fe3+ is the oxidizing agent

33

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

34

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

35

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

36

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

1.36

37

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

3.16x10-4

38

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

39

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

40

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

3.03

41

Emission

going from a higher energy state to a lower energy state

Energy is emitted

42

Absorption

going from a lower energy state to a higher energy state

Energy is absorbed

43

what does a Long wavelength entail?

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

44

What does a Short wavelength entail?

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

45

ionization energy

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

46

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

47

isoelectronic

having the same number of electrons

48

Which of the following are isoelectronic with Cl-?

1. Ca2+
2. S2-
3. O2-

Ca2+ and O2-

49

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

50

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

1

51

Hund's Rule

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

52

Aufbau Principle

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

53

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

54

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

1

55

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

56

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

57

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

1.12

58

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

59

m to nm

10^9

60

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

61

What is the ground state electron configuration for Cr2+?

[Ar] 3d4

62

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

I

Mn

S

Ge

Sr

Sr

63

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

64

electromagnetic spectrum order

low wavelength to high wavelength

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

65

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

NO3 – only

66

Which species is reduced in the reaction below?

I–(aq) + ClO–(aq) → IO–(aq) + Cl–(aq)

ClO-

67

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

energy, frequency, wavelength

long line: more energy, high frequency, low wavelength

68

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

energy, frequency, wavelength

short line: less energy, less frequency, high wavelength

69

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

atoms get bigger

70

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

atoms get smaller

71

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)

72

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

1-n = 3, l = 1, ml = ?1, ms = +1/2
2-n = 3, l = 2, ml = ?3, ms = +1/2
3-n = 4, l = -1, ml = ?1, ms = +1/2
4-n = 4, l = 2, ml = ?2, ms = +1/2
5-n = 4, l = 1, ml = ?2, ms = +1/2

2,3,5

73

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

4.64E+14 s-1

74

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

shape of orbital

75

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

3s

76

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

K+ Cl-

77

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

+4, +7