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Chem! > Matter and Energy > Flashcards

Matter and Energy Flashcards

1
Q

Matter

A

Anything that takes up space of volume and has mass

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2
Q

Pure substances

A

Elements and compounds

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3
Q

Elements

A

Substances that cannot be broken down or decomposed into simpler substances by chemical means

Ex: H2(g), Ne(g)

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4
Q

Compounds

A

2 or more different elements chemically bonded together

LiH(s), NaCO3(s)

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5
Q

Binary compound

A

Contains 2 different elements

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6
Q

Ternary compound

A

Contains 3 different elements

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7
Q

Mixtures

A

Homogenous and heterogeneous

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8
Q

Homogenous mixture (solution)

A
  • Observe 1 distinct phase
  • Particles are uniformly dispersed
  • Clear, transparent
  • Cannot be filtered

Ex: NaCl(aq), CuSO4(aq)

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9
Q

Heterogenous mixture

A
  • Observe 2 or more distinct phases
  • Particles are unevenly dispersed
  • Not clear and not transparent
  • Can be filtered

Ex: Greek salad, oil and water, soil

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10
Q

How do you remove salt from water?

A

Heat the solution in order to evaporate out the water and be left with salt

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11
Q

Physical properties

A

Observed using 5 senses

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12
Q

Examples of physical properties

A

Texture, taste, shape, color, smell, phase of matter, density, solubility

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13
Q

Physical properties of metals

A

Luster, conductivity, malleability, ductility, tenacity

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14
Q

Why do metals conduct electricity?

A

Due to a sea of mobile electrons

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15
Q

Malleability

A

Can be hammered into sheets

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16
Q

Ductility

A

Can be drawn into wires

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17
Q

Tenacity

A

Strength

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18
Q

Physical change

A

A change that does not alter the chemical properties of the substance

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19
Q

Phase changes

A

A type of physical change

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20
Q

Melting

A

Solid to liquid

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21
Q

Evaporation

A

Liquid to gas

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22
Q

Sublimation

A

Solid to gas

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23
Q

Freezing/solidification

A

Liquid to solid

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24
Q

Condensation

A

Gas to liquid

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25
Deposition
Gas to solid
26
Chemical properties
Describe how a substance reacts
27
Examples of chemical properties
Inert (noble gases), radioactivity, acidity, flammability, combustibility, rust, sours, spoils
28
What substances sublime readily?
Iodine and carbon dioxide (dry ice)
29
Which substance is flammable?
Hydrogen
30
Which substance is combustible?
Methane
31
Which substance supports combustion but is not combustible?
Oxygen
32
Chemical changes
Production of new substances through a reaction
33
Potential energy
Stored energy
34
Kinetic energy
Energy of motion
35
6 other types of energy
1) Thermal (heat) 2) Solar (sun) 3) Nuclear 4) Mechanical (pulley, lever) 5) Chemical (batteries) 6) Electrical
36
Law of conservation of energy
Energy cannot be created or destroyed, it can only change its form
37
Energy units
- calorie/kilocalorie - joule/kilojoule 1 calorie = 4.18 joule
38
When bonds are broken,
Energy is absorbed
39
When bonds are formed,
Energy is released
40
Where is energy stored?
In bonds between atoms
41
Endothermic reaction
Heat is absorbed and the walls of the container become cool
42
Exothermic reaction
Heat is released and the walls of the container become warm
43
Is a combustion reaction endothermic or exothermic?
Exothermic
44
Temperature
A measure of a substance’s kinetic energy
45
Freezing/melting point
0°C and 273K
46
Boiling/condensation point
100°C and 373K
47
Absolute zero
All motion stops at 0K
48
Celsius to kelvin conversion
°C + 273 = K
49
Kelvin to celsius conversion
K - 273 = °C
50
Endothermic phase changes
Melting, evaporation. sublimation
51
Exothermic phase changes
Freezing, condensation, deposition
52
Direction of heat flow
Heat flows from the hotter object to the colder object
53
Phase changes take place at…
Constant temperatures
54
Potential energy increases as…
The distance between particles increases
55
Reaction coordinate
The path that a reaction takes
56
Activation energy
Minimum amount of energy that must be added to the reactants to start the reaction
57
Activated complex
Intermediate stage between reactants and products, transition species
58
Heat of the reaction, delta H, or enthalpy
Heat of the products - heat of the reactants
59
If the heat of the reaction is positive, the reaction is…
Endothermic
60
If the heat of the reaction is negative, the reaction is…
Exothermic
61
How does a catalyst affect the potential energy diagram?
1) Provides an alternate pathway 2) Decreases the activation energy of the forward and reverse reaction 3) Decreases the energy of the activated complex *Doesn’t affect enthalpy
62
Calorimetry
The science of measuring heat lost or gained in a reaction
63
Calorimeter
Device used to measure energy changes
64
Specific heat capacity
For every one gram of water, 4.18 J of heat must be added to raise the temperature by 1°C
65
Why do metals have low specific heats?
They are conductors of heat and electricity
66
Specific heat capacity formula
q = m C delta T
67
Why can’t we use the formula q = m C delta T for phase changes?
There is no change in temperature, so delta T = 0°C
68
Heat of fusion
Melting and freezing
69
Heat of fusion formula
q = mHf
70
Heat of vaporization
Boiling and condensation
71
Heat of vaporization formula
q = mHvap

Chem! (9 decks)

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