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Chm 1046 > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

Atoms interact…..

A

Electrostatically

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2
Q

Interactions range from….

A

LDF to bonding

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3
Q

When atoms interact, the system becomes more….

A

Stables and loses energy to surrounding

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4
Q

All electrostatic interactions require

A

Energy to overcome

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5
Q

The way atoms interact depends on the…..

A

Arrangement of electrons

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6
Q

When atoms form a new compound the properties are?

A

Emergent

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7
Q

Properties of materials depend upon

A

-the type of bonds
-spatial arrangement of atoms
-interactions between molecules

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8
Q

Temperature of phase changes allows us to make

A

Predictions about type of infections.

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9
Q

A change of 1 C equals

A

A change of 1 k

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10
Q

0 Celsius equals

A

273.5 k

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11
Q

0 kelvin equals

A

Absolute zero

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12
Q

What does temperature tells us?

A

The directions thermal energy or heat will move

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13
Q

Energy always move from

A

Higher temperature to lower temperature

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14
Q

Thermal energy depends on

A

How much material you have

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15
Q

Temperature depends on

A

The average ke of the particle

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16
Q

At the molecular scale we usually consider

A

Populations (lots of particles)

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17
Q

One molecule can have a…. But not a

A

Ke……temperature

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18
Q

Populations of molecules have a temperature where

A

Average ke=1/2 mv^2=3/2 kt

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19
Q

What happens to the average velocity of a gas if the temperature increases?

A

Increases

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20
Q

If the molar mass of the gas increases, what happens to the average velocity?

A

Decreases

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21
Q

Energy associated with motion of particles is

A

Thermal energy

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22
Q

Is the transfer of thermal energy from one place to another (eg by collision of molecules)

A

Heat

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23
Q

Is how much energy it takes to change the temperature of a substance?

A

Specific heat/ heat capacity

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24
Q

Energy required to raise 1 g by 1 c (or 1 k)

A

Specific heat

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25
Energy required to raise 1 mol by 1 c (or 1 k)
Molar heat capacity
26
Which substance would increase in temperature the most when the same amount of thermal energy is added to 1 g of each substance (water, methanol, ethanol, and propanol)
It would be propranolol because it has the lowest specific heat.
27
Which substance will reach the highest temp if the same amount of heat is added to 10g of each? Water, steam, silver, iron, aluminum, copper
Silver because of it low specific heat
28
Which will end up at the lowest temperature? Between water, steam, aluminum and silver or copper
Water
29
Does steam have IMFs? Which ones are they
Yes, LDF, Hydrogen Boning and Dipole-Dipole.
30
As……. Is added it can increase kinetic energy and be used to overcome IMFs in the substance.
Energy
31
When we add energy to water what happens to the temperature
It increases.
32
What is the mechanism of adding thermal energy?
Collision
33
When molecules have more energy what is the consequences?
Move faster: translate, vibrate and rotate
34
Measuring the changes in …….. give us evidence about what is happening at the molecules level
Temperature.
35
Phase change? Move from
Solid—->liquid—->gas Gas—->liquid—->solid
36
During a phase change what happens to temperature?
Does not changes
37
When would temperature change?
After the phase change is complete.
38
When……………… or ………………., energy is added from the surroundings and used to overcome the IMFs between the molecules (or ions)
Melting or boiling
39
When…………… or ……………….., energy from the formation of new interactions is being released into the surrounding
Condensing or freezing.
40
In exothermic reaction heat is
Released
41
In exothermic reaction the sign on heat will be
Negative
42
In endothermic reaction heat is
Absrobed
43
In endothermic reaction the sign on heat will be
Positive
44
The formation of bonds can be considered a
Exothermic process
45
The breaking of bonds can be considered a
Endothermic process
46
Heat absorbed by the system is
Endothermic (+)
47
Heat is released by the system is
Exothermic (-)
48
Work done on the system by the surrounding
Decreases and is positive
49
Work done by the system on the surrounding
Increases and is negative
50
Can transfer matter and energy
Open system
51
Transfer energy but not matter
Closed system
52
No transfer of matter or energy
Isolated system
53
State functions depends on
The initial and final state
54
Path function depends on
How change takes place
55
Sum of all the ke and pe of all particles in the system
Internal energy
56
What can internal energy E calculate
The change in delta E
57
Heat absorbed or emitted during a reaction under constant pressure is
Enthalpy or H
58
If delta H is positive the reaction is
Endothermic
59
When delta h is endothermic what happens
Heat goes into the reaction and the surrounding gets cold
60
If delta h is negative the reaction is
Exothermic
61
What happens when delta h is exothermic
Heat goes out of the reaction and the surrounding gets hot.
62
Is wood burning an exothermic or endothermic reaction
Exothermic
63
is water freezing and exothermic or endothermic reaction
Exothermic
64
Is sweat evaporating an endothermic or exothermic reaction
Endothermic
65
Is chemical hand-warmer an exothermic or endothermic reaction
Exothermic
66
What does the thermal energy change q depends on
The mass of substance, the temperature change and the specific heat Q= m x c x delta t

Chm 1046 (2 decks)

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