Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chem > Final Review > Flashcards

Final Review Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

How would you describe the Bohr Model of the atom?

A

electrons orbit the nucleus in shells (planetary model) + energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

How did the quantam mechanical model improve on the Bohr model?

A

It says that electrons do not orbit the nucleus, but in other regions of space. We only know the probability of finding electrons in these spaces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Describe the most current theory of the atom’s structure

A

large nucleus that contains neutrons & protons. Electrons exist around the nucleus in clouds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

How are protons and electrons related in a neutral atom? How are they related in a charged atom?

A

Neutral - equal
Charged - one is more than the other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What conclusion about the atom was made from Rutherford’s gold foil experiment?

A

atoms are mostly empty space with a dense, positive, small nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Describe the change in movements when electrons become “excited”

A

They jump up energy levels farther from the nucleus & become very unstable. Energy is absorbed as electrons move to higher energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What causes color bands to be emitted?

A

As electrons become relaxed, they fall back to ground state and release the energy they absorbed into light and heat

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the total number of electrons in all s orbitals of a neutral atom of phosphorous

A

6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

How many valence electrons are in 1s^2,2s^2,2p^6, 3s^2, 3p^6, 4s^2

A

2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the maximum number of electrons that can occupy the 2nd energy level

A

8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What shape best represents the p orbital?

A

peanut / dumbbell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is the electron config for an atom of germanium at ground state

A

check 19 in packet

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

what is the electron config for potassium atom at ground state

A

check 20 in packet

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Draw an orbital diagram for the s-block elements in the third period

A

check 21 in packet

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What type of nuclear decay is
4
He
2

A

Alpha

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What type of nuclear decay is
0
e
-1

A

beta

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

which nuclear process decreases the atomic number by 1

A

beta

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

which nuclear process decreases the atomic mass by 4

A

alpha

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

The half-life of phosphorous is 14.3 days. How many mg of a 20 mg sample will remain after 85.8 days

A

.3125

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

When 42 / 19 K undergoes radioactive decay, the result is 2 products, one of which is calcium - 42. What is the other product?

A

0
e
-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

How are 2 atoms that are isotopes of the same element different from one another?

A

Different #s of neutrons and mass #s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

How does Ga become a +3 ion

A

it loses 3 e-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Describe how 2 atoms in a covalent bond are both attracted to and repelled by one another

A

shared e- are attracted, the lone pair repels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What are the 2 different ions present in the compound Li3N?

A

Li+ , N3-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Is Mg(NO3)2 best classified as ionic or molecular?

A

ionic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What two properties are typical of molecular compounds?

A
  • gases or liquids at room temp
  • atoms share electrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Which part of the atom is most directly involved in chemical bonding

A

electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What is the benefit of using pure iron filings instead of a pure iron nail to conduct a chemical reaction involving iron

A

more surface area makes filings more reactive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

List these four elements from smallest to largest atomic radii: Cl, P, Si, S

A

Cl, S, P, Si

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What property of elements is used to calculate the degree of polarity of a covalent bond between 2 atoms?

A

Electronegativity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Which element on the periodic table has the highest electronegativity

A

F

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What causes a solution to become saturated

A

The maximum amount of solute has dissolved

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

When a solute is added to a solvent, how will the boiling point, freezing point, and vapor pressure be changed?

A

Boiling point increases, freezing point decreases, vapor pressure decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Equal concentration solutions of sodium chloride, aluminum chloride, magnesium nitrate, and aluminum sulfate are prepared. Which solute would be expected to cause the greatest change in boiling point compared to the pure solvent?

A

Al2SO43, because it has the most particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

What are 3 ways to increase the solubility of most solid solutes?

A

Increase temperature, increase surface area, increase agitaiton

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

What lab technique is best to seperate a solid from a liquid to recover the liquid

A

filtration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

What physical property of substances is used in distillation to separate a mixture of liquids

A

boiling point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

What is the formula for molarity?

A

n / L

39
Q

what is the molarity of a 0.5 L sample of a solution that contains 60g of sodium hydroxide

A

3

40
Q

Describe how to identify a base vs an acid by looking at the chemical formula

A

Base has OH, acids have H

41
Q

What will happen to NaOH when phenolphthalein is added?

A

pink

42
Q

What will happen to HCl when phenolphthalein is added?

A

colorless

43
Q

what will happen to NH3OH when phenolphthalein is added?

A

pink

44
Q

what will happen to NaCl when phenolphthalein is added?

A

Clear, bc its a salt

45
Q

Tell whether each substance is polar or non-polar:
Water
Ammonia
Methane

A

Water: P
Ammonia: P
Methane: NP

46
Q

The intermolecular forces present in HSCH2CH2SH

A

dipole-dipole
dispersion

47
Q

Which pairs represent liquid combinations that will mix homogeneously?
Octane (C8H18) & H2O
Acetic Acid (CH3COOH) & H2O
Octane & Carbon Tetrachloride

A

Pair 2 &3 - if a compound is only carbons and hydrogens, it’s non-polar!

48
Q

Why would C8H18 be soluble in CCl4, but NaCl wouldn’t be soluble in CCl4?

A

C8H18 are both NP, water is polar

49
Q

What is the molecular geometry of PI3?

A

trigonal pyramidal

50
Q

Molecular geometry of water

A

bent

51
Q

molecular geometry of CO2

A

linear

52
Q

molecular geometry of ammonia (NH3)

A

trigonal pyramidal

53
Q

molecular geometry of methane (CH4)

A

tetrahedral

54
Q

Identify 2 characteristics of an exothermic reaction that differs from that of an endothermic reaction

A

Releases heat to surroundings, -delta H

55
Q

Which changes in phase would be considered exothermic?

A

Freezing, condensation, deposition

56
Q

Fundamental Units

A
  • independent of other units
  • meter, second, kg, candela, ampere, kelvin, mole
57
Q

Derived Units

A
  • pressure, density, volume, velocity, force, energy
  • found by multiplying, dividing, etc fundamental units
58
Q

Difference between physical & chemical properties

A

physical can be observed without performing a reaction, while chemical can be observed during or after a reaction

59
Q

Which phase has the strongest IMFs?

A

solids

60
Q

Which phase diffuses an immeasureable amount?

A

solid

61
Q

Which phase diffuses easily but slowly

A

liquid

62
Q

which phase has no IMFs?

A

gas

63
Q

which phase has vibrations only of molecules?

A

solid

64
Q

Which phase diffuses easily and quickly?

A

gases

65
Q

Formula for density

A

m / v

66
Q

A student found a sample of an unknown liquid in the lab station cabinet. After experimentation, he found that the substance had a density of 1.65 g/mL. Will it float in water?

A

An object that is less dense than water will float, so no. 1.65 g/mL > 0.999 g/mL

67
Q

Formula for volume?

A

m / d

68
Q

Scientific Notation of Kilo

A

1 x 10 ^3

69
Q

Scientific Notation of Centi

A

1 x 10 ^-2

70
Q

Scientific Notation for Milli

A

1 x 10^-3

71
Q

Scientific Notation for Micro

A

1 x 10^-6

72
Q

Scientific Notation for Nano

A

1 x 10 ^-9

73
Q

Accuracy

A

the degree of closeness of measurements to the true or accepted value

74
Q

Precision

A

the degree to which repeated measurements under changed conditions show the same result.

75
Q

How much water would form if 59.7 g of H reacted with 140.4 g of O

A

200.1

76
Q

Formula for kinetic energy

A

0.5 (m)(v)^2

77
Q

C –> K

A

+273

78
Q

K –> C

A
  • 273
79
Q

What happens to temperature during phase changes?

A

it stays constant

80
Q

5 postulates of kinetic molecular theory

A

1) Gases are mostly empty space because the separation is more than the size of the molecules.
2) Collisions with the sides of the container are more frequent & less frequent with each other. Collisions are elastic.
3) Particles move in a straight direction & randomly
4) Particles attract & repel because they don’t have any sense of IMFs
5) the average kinetic energy of all particles in a sample is proportional to temp

81
Q

Boyle’s Law

A

P1V1 = P2V2. Pressure and volume have an indirect relationship.

82
Q

Charles’ Law

A

V1/T1 = V2/T2. Direct relationship.

83
Q

Gay-Lussac’s Law

A

P1/T1 = P2/T2

84
Q

Dalton’s Law of Partial Pressure

A

Ptot = Pa + Pb + Pc

85
Q

Ideal Gas Law

A

P = nrt

86
Q

What would be the density of oxygen gas at 70 C and 3 atm?

A

Use MM = drt / p

87
Q

Aufbau Principle

A

Electrons are placed in orbitals of lowest energy 1st

88
Q

Pauli Exclusion Principle

A
  • orbitals can hold 2 e-
  • no 2 #s can have the same quantam numbers
  • arrows have to have opposite spins
89
Q

Hund’s Rule

A

when filling a sublevel, one e- enters each orbital until it’s full, then they pair

90
Q

Isoelectronic

A

Same # of electrons

91
Q

Lanthinides

A

1st row of box under table

92
Q

Actinides

A

2nd row of box under table

93
Q

How do you find something’s degree of polarity?

A

Find the difference between electronegativities

Chem (15 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions