Brainscape's Knowledge GenomeTM

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


See full index

Chemistry 121 > Exam 3 blocks 7-9 > Flashcards

Exam 3 blocks 7-9 Flashcards

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

What does chemical arithmetic allow?

A

It allows us to us the information provided by balanced chemical equations to describe chemical reactions in two ways
Qualitative and quantatative

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

What is formula mass?

A

the sum of all of the atomic masses of all atoms in its chemical formula

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

What is the conversion factor for converting amu’s into grams

A

1.000amu=1.660x10^-24g

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

What are the two ways that quantity of a sample can be expressed?

A

mass of a sample

number of objects in a sample

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

How much is one mole of something?

Avogadro’s number

A

1 mole=6.02x10^23

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

Is Avogadro’s number exact?

A

yes

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

to find out how many atoms in a mole?

A

we multiply by Avo’s number

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

To find out how many moles from a number of atoms?

A

We divide by Avo’s number

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

What is Molar mass?
what is its abbreviation?
Unit expression?

A

The mass of one mole of an object
MM
Grams per mole, g/mole, g-mole^-1

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

How do we find the molar mass of an element?

A

it is the same as the amu off the periodic table just expressed in grams

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

How would we find the find the mass of a single atom of an element that is expressed in grams per mole?

A

we would divide the MM by Avo’s number

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

How would we find out the mass of one mole of an element in amu’s?

A

multiply the amu by Avo’s number

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

how do we convert formula mass to compound molar mass?

A

change the units from amu to g

no conversion required

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

Why is it that we can switch from amu to g without a conversion?

A

The definition of a mole + the fact hat amu is baised off of C-12

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

What is a Mole?

A

The amount of a substance in a system that contains as many elemental particles as there are atoms in exactly 12 grams of C-12

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

What is the ever repeating core in chemical calculations?

A

Number of moles of the the substance times time the number of moles of the specific element in the substance over one more of the substance

example, How many moles of O in a 1.5 mole sample of CO2
2 Moles of O
1.5 moles of CO2 X —————— = 3.0 moles of O
1 Mole of CO2

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

What is a chemical equation?

A

A written statement that uses symbols instead of words to describe the changes that occur as chemical reaction proceed

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

What is (s) mean in a chemical equation?

A

solid

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

What is (g) mean in a chemical equation?

A

gas

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

What is (l) mean in a chemical equation?

A

dissolved in some liquid

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

What is (aq) mean in a chemical equation?

A

dissolved in water

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

What is stoichionmetry

A

Stoichiometry the application of the laws of definite proportions and the conservation of mass and energy to chemical activity

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

What does the concept of mass balance require?

2 things

A

all atoms present as reactants MUST also be present as products

all atoms present as products MUST also be present as reactants

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

The law of conservation of matter dictates…….

A

That mass balance must be observed in chemical reations

mass can neither be created or destroyed in ordinary chemical reactions and changes

reactants simply rearrange themselves into new substances (products) in chemical reactions

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

What is the chemical equation for the haber process?

What is this process describing?

A

N2(g)+3H2(g)——> 2NH3(g)

Nitrogen fixing makes N2 bio-available

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

What is the balanced equation for the thermite reaction?

A

2Al(s)+Fe2O3(s)—–>2Fe(s)+Al2O3(s)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Secondary forces aka…

A

intermolecular forces

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

where do secondary intermolecular forces occur?

A

between function between the fundamental particles within a system

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

The prefix Inter means?

A

between

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

What substance has a total absence of intermolecular forces?

A

ideal gasses

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

Intermolecular forces are dominate in ___

A

solids

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

intermolecular forces are nonexistent in ____

A

ideal gasses

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

Inter and intra-molecular forces are equal in_____

A

liquids

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

What is the formula for kinetic energy?

A

KE=1/2mXv^2

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

What does KMTM stand for?

A

The Kinetic Molecular Theory of Matter

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

What is the KMTM

A

5 statements Based on the fact that all fundamental particles in a system are always in motion regardless of their physical state

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

What is the first statement of the KMTM

A

Fundamental particles that compose matter have definite and characteristic sizes

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

What is the second statement of the KMTM

A

The fundamental particles in any system possess a certain amount of kinetic energy in the form of constant random motion.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

Why is kinetic energy considered a disruptive force in matter?

A

The random constant motion of the fundamental particles cause them to move further and further apart from one another decreasing the stability of the system. Weakening the matter.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

What is the third statement of the KMTM

A

The atoms and molecules in any syatem also possess certain amount of potential energy stored in two possible forms

intramolecular force stored in chemical bonds

in covalent bonds PE is present in intermolecular forces as well *much weaker

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

Why is potential energy considered a cohesive force.

A

Potential energy pulls particles in a system closer together and increases the stability of the system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

Where does the potential energy come from?

A

Electrostatic interactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

Where can PE be found in ionic compounds?

A

only in intramolecular forces of covalent compounds have PE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

Where can PE be found in covalent compounds?

A

IN both the inter and intra-molecular forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

What is the fourth statement of the KMTM?

A

The velocity of the particles in a system is temperature dependent

The higher the temp the faster the particles move the more KE produced

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

What is the fifth statement of the KMTM?

A

As particles in the system collide with eachother via “elastic collisions” they will transfer KE between themselves.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

What are elastic collisions?

A

Hypothetical collisions in a system where energy is conserved within a system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

particles in a system refereed to as hot have ____ KE

A

higher

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

particles in a system refereed to as cold have ____ KE

A

lower

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

What is the overall statement of the KMTM?

A

to explain the differences in states of matter in terms of the disruptive(KE) and cohesive(PE) forces present

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

When does kinetic energy equal 0?

A

never even the most solid matter will have some KE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

When doe PE equal 0?

A

only in ideal gasses

53
Q

What is an ideal gas?

A

a hypothetical gas in which cohesive forces are nonexistent. all collisions are elastic

54
Q

What gasses can be considered idea?

A

Virtually all of them.

Because at room temp. the cohesive forces as so close to 0 they can be taken out of the equation

55
Q

Reducing temperature reduces ___energy

A

kinetic

56
Q

increasing temperature increases _____energy

A

Kinetic

57
Q

When will ideal gasses show “real” behavior?

A

if intermolecular forces are allowed to form…AKA temperature reduction or a pressure increase leads to increased intermolecular cohesive forces

58
Q

A gas is compressed when….

A

the size of its container is decreased but the number of gas particles is not.

59
Q

pressure increase from compression occurs because?

A

the particles have more frequent collisions with the sides of the container

60
Q

What are three ways to increase pressure?

A

Compression, Temperature increase, and adding more gas to the same container

61
Q

pressure =?

A

the number of collisions with container

62
Q

What are gas laws?

A

mathematical expressions that describe the relationships between variables in gasses

63
Q

What are the 4 variables in gas laws?

A

of moles (n)

Pressure (P)
Volume (V)
Temperature (T)

64
Q

What does the subscript “1” mean in a gas law?

A

starting condition

65
Q

What does the subscript “2” mean in a gas law?

A

ending condition

66
Q

What is Boyles law and what does it state?

A

An inverse pressure-volume relationship

states that the pressure of a gas is inversely proportional to the volume occupied by the gas when the number of moles and temperature are constant

67
Q

What is boyles law equation?

A

P1xV1=P2xV2

68
Q

What is charles law and what does it state?

A

A temp-volume direct relationship

states that the temp of a gas is directly proportional to the volume it occupies when moles and pressure are the same

69
Q

What is charles law equation?

A

T2xV1= T1xV2

70
Q

What is the combined gas law?

When is it used?

A

a simple mathematical combination of boyles and charles law in which temp nor pressure need to be held constant

When volume, temp, and pressure are all changing

71
Q

What unit does the temp. in the combined gas law need to be in?

A

K

72
Q

What is the ideal gas equation?

what two conditions need to be met to use it?

A

you are working with only one constant set of P,V,T conditions

the number of Moles(n) is changing

73
Q

What units does T need to be in for the ideal gas law equation?

A

Kelvin

74
Q

What units does P need to be in for the ideal gas law equation?

A

Atmospheres

75
Q

What units does V need to be in for the ideal gas law equation?

A

Liters

76
Q

What units does n need to be in for the ideal gas law equation?

A

moles

77
Q

What is the R variable in the ideal gas law

A

the universal gas constant.

R= 0.0821 L x atm x mol^-1 x K^-1

78
Q

How many in. Hg is in one atm?

A

1.000 amt=29.92 in

79
Q

how many mm Hg in one atm

A

1.000 amt=760.0mm

80
Q

How many torr in one atm?

A

1.000 amt=760.0 torr

81
Q

how many PSI in one atm

A

1.00 amt= 14.7 PSI

82
Q

How many bars in one atm

A

1.00 atm = 1.01 bar

83
Q

What is the substitution for n in the ideal gas equation?

A

g
n=——–
mm

84
Q

In chemistry what does STP stand for?

A

standard temp and pressure

0 degrees C and 1 atm pressure

85
Q

In chemistry what does RTP stand for?

A

Room tempature and pressure

25 degrees C and 1 atm pressure

86
Q

What is the standard molar volume of any ideal gas at STP?

A

22.4 L

87
Q

what are intermolecular(secondary) forces

A

forces that occur between fundamental particles

88
Q

what are intramolecular(primary) forces?

A

forces that occur within fundamental particles (chemical bonds) and are much stronger than intermolecular forces

89
Q

in what state of matter do intermolecular forces have the largest effect? and why?

A

bother inter and intra forces are significant in liquids.

only in liquids do the intermolecular forces cause dramatic effects.

90
Q

how do intermolecular forces have an effect on the behavior of matter if they are so weak?

A

because they may be weak but they are additive throughout the system

91
Q

What are the three intermolecular forces in liquids? list in order of strongest to weakest retaliative to single interactions

A

Hydrogen bonds
dipole-dipole
London forces

92
Q

What is a Dipole-dipole interaction?

A

and electrostatic attraction between polar molecules

93
Q

how is the boiling point of a liquid affected by the presence of dipole dipole interactions?

A

the boiling point is increased by the presence of dipole dipole interactions as they increase the cohesive forces within the liquid because the collective attraction of the forces increase the strength and stability of the liquid

94
Q

What is hydrogen bonding?

A

an extremely strong dipole dipole interaction

95
Q

is a hydrogen bond a type of chemical bond?

why/why not?

A

No

because it occurs between fundamental particles and it is nowhere near as strong

96
Q

What are the only elements that can be involved in H bonding?
why?

A

F H O N

they are small and highly electronegative appart from H

97
Q

What are the two criteria for H Bonding?

A

1- one of the members of the bond must be a hydrogen atom contently bonded to a very small AND highly electronegative atom (F, O, N)

2-the other member of the bond must be a small AND highly electronegative atom that also has a lone pair of electrons

98
Q

Why is H bonding so important for life?

A

it is extremely significant in aqueous systems. and all life as we know it is aqueous

99
Q

Explain the process of H bonding

A

Hydrogen contently bonds with either F, O, N.
The extreme difference in electronegativity causes hydrogen’s sole electron to become so attracted to the electronegative atom that the hydrogen’s nucleus becomes almost bare

the “bare” nucleus becomes attracted to the lone pair of the other molecule an is small enough to come very close to it. increasing the strength of the attraction

100
Q

What is the other word for london forces?

A

van der Waals forces

101
Q

what are london forces?

A

the weakest of all intermolecular forces, london forces which can occur in all covalent systems.

they are forces formed by the movement of electrons.

102
Q

Explain london forces

A

electrons in a covalent system can be anywhere in the electron cloud at any given time. when the electrons (even for an instant) leave the favorable center of the bond they form an instantaneous dipole

103
Q

what is an instantaneous dipole

A

when a bond becomes polarized due to the electrons in the bond leaving the favorable position in a covalent bond.

happens near the speed of light

104
Q

what happens to adjacent molecules when london forces occur?

A

they all respond by either attracting or repelling the charge

the single formation of a dipole cause a chain reaction so that all other molecules in the system must react as well.

105
Q

what does it mean for london forces to be transitory?

A

they switch on and off

106
Q

what is evaporation?

A

a process in which molecules escape from the liquid phase and enter the gas phase

107
Q

what are vapor molecules?

A

evaporated molecules

108
Q

what are the three criteria for evaporation?

A

1-the molecules kinetic energy must be stronger than the cohesive forces
2-the molecules movement must be favorable for escape
3-the molecule must be close to the surface

109
Q

what effects the rate of evaporation?

A

the exposed surface area

the temperature

110
Q

what are the two type of equilibrium?

A

static and dynamic

111
Q

what are the effects of evaporation on the liquid phase?

A

volume decrease

tempature decrease

112
Q

define dynamic equilibrium

A

a condition which two processes which are exact opposites of each other are occurring at exactly equal rates so the net charge of the system equals zero

113
Q

what is an example of dynamic equilibrium?

explain

A

evaporation in a sealed container
as the molecules vaporize and fill the head space, it becomes more and more crowded. the collision of the vapor molecules in the head space cause some of them to loose enough kinetic energy to be below the level needed to escape in the first place. as random moments occur, once the molecule with low kinetic energy touches the surface of the liquid it condolences back into the liquid

114
Q

what do dynamic equilibrium systems appear static

A

because everything is changing at equal rates

115
Q

how are vapor pressure and evaporation related?

A

if the vapor pressure of a liquid is greater than the attm the liquid will evaporate

116
Q

what makes a liquid volatile?

A

high vapor pressure

117
Q

what is boiling point in terms of pressure?

A

when the vapor pressure is they same as the attm pressure the liquid will boil

118
Q

where does the change of state occur in boiling liquids?

A

inside the bubbles that are formed

119
Q

why does the temperature of a boiling liquid stay constant regardless of how much heat is applied?

A

because the bubbles formed when boiling develop a dynamic equilibrium
the heat lost in evaporation is equal to the amount of heat the liquid gains through condensation

120
Q

the charge of ferric

A

III

iron III

121
Q

the charge of ferrious

A

II

iron II

122
Q

the charge of Cupric

A

II

copper II

123
Q

the charge of cuprous

A

I

copper I

124
Q

cobaltic

A

III

cobalt III

125
Q

cobaltous

A

II

cobalt II

126
Q

stannic

A

IV

tin IV

127
Q

stannous

A

II

tin II

128
Q

plumbic

A

IV

Lead IV

129
Q

plumbous

A

II

lead II

Chemistry 121 (6 decks)

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