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Chm 1046 > Chapter 5 > Flashcards

Chapter 5 Flashcards

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
Q

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

A

Molar heat capacity

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26
Q

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)

A

It would be propranolol because it has the lowest specific heat.

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27
Q

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

A

Silver because of it low specific heat

28
Q

Which will end up at the lowest temperature? Between water, steam, aluminum and silver or copper

A

Water

29
Q

Does steam have IMFs? Which ones are they

A

Yes, LDF, Hydrogen Boning and Dipole-Dipole.

30
Q

As……. Is added it can increase kinetic energy and be used to overcome IMFs in the substance.

A

Energy

31
Q

When we add energy to water what happens to the temperature

A

It increases.

32
Q

What is the mechanism of adding thermal energy?

A

Collision

33
Q

When molecules have more energy what is the consequences?

A

Move faster: translate, vibrate and rotate

34
Q

Measuring the changes in …….. give us evidence about what is happening at the molecules level

A

Temperature.

35
Q

Phase change? Move from

A

Solid—->liquid—->gas
Gas—->liquid—->solid

36
Q

During a phase change what happens to temperature?

A

Does not changes

37
Q

When would temperature change?

A

After the phase change is complete.

38
Q

When……………… or ………………., energy is added from the surroundings and used to overcome the IMFs between the molecules (or ions)

A

Melting or boiling

39
Q

When…………… or ……………….., energy from the formation of new interactions is being released into the surrounding

A

Condensing or freezing.

40
Q

In exothermic reaction heat is

A

Released

41
Q

In exothermic reaction the sign on heat will be

A

Negative

42
Q

In endothermic reaction heat is

A

Absrobed

43
Q

In endothermic reaction the sign on heat will be

A

Positive

44
Q

The formation of bonds can be considered a

A

Exothermic process

45
Q

The breaking of bonds can be considered a

A

Endothermic process

46
Q

Heat absorbed by the system is

A

Endothermic (+)

47
Q

Heat is released by the system is

A

Exothermic (-)

48
Q

Work done on the system by the surrounding

A

Decreases and is positive

49
Q

Work done by the system on the surrounding

A

Increases and is negative

50
Q

Can transfer matter and energy

A

Open system

51
Q

Transfer energy but not matter

A

Closed system

52
Q

No transfer of matter or energy

A

Isolated system

53
Q

State functions depends on

A

The initial and final state

54
Q

Path function depends on

A

How change takes place

55
Q

Sum of all the ke and pe of all particles in the system

A

Internal energy

56
Q

What can internal energy E calculate

A

The change in delta E

57
Q

Heat absorbed or emitted during a reaction under constant pressure is

A

Enthalpy or H

58
Q

If delta H is positive the reaction is

A

Endothermic

59
Q

When delta h is endothermic what happens

A

Heat goes into the reaction and the surrounding gets cold

60
Q

If delta h is negative the reaction is

A

Exothermic

61
Q

What happens when delta h is exothermic

A

Heat goes out of the reaction and the surrounding gets hot.

62
Q

Is wood burning an exothermic or endothermic reaction

A

Exothermic

63
Q

is water freezing and exothermic or endothermic reaction

A

Exothermic

64
Q

Is sweat evaporating an endothermic or exothermic reaction

A

Endothermic

65
Q

Is chemical hand-warmer an exothermic or endothermic reaction

A

Exothermic

66
Q

What does the thermal energy change q depends on

A

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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