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Chemistry > Unit 1: Matter > Flashcards

Unit 1: Matter Flashcards

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1
Q

Chemistry is

A

the science concerned with properties, composition, and behaviour of matter
- Essentially the study of matter

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2
Q

Mass is

A

the amount of matter contained in a thing

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3
Q

Extensive properties

A

qualities that are dependent on the amount of the material

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4
Q

Intensive properties

A

qualities that do not depend on the amount of material

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5
Q

Extensive or intensive: price of one pound of apples is $4.99

A

intensive

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6
Q

Extensive or intensive: Diya bought some apples for tonight

A

Extensive

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7
Q

KEY WORDS for determining intensive properties

A

if the sentence says: per pound, per gram, etc = intensive property

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8
Q

potential energy is

A

the amount of freedom particles have to move.
–> acc def: the energy of the intermolecular forces between the particles —> rmr the card about attraction and energy state

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9
Q

latent heat is

A

the heat that is being used in phase change.
Latent heat comes into the system from the outside –> which increases the PE

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10
Q

physical or chemical properties: Which property can be determined without changing the identity(creating a new substance) of the substance?

A

physical properties

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11
Q

chemical properties

A

are properties that hold the ability to change the identity of the substance –> must cause a new substance to form. they cause a reaction.
- flammability
- toxicity
- ability to oxidize
- heat of combustion

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12
Q

physical properties

A

properties that you can measure and observe without changing the substance itself. A lot of them describe the relation & interaction between matter and energy (ex, magnetic property)
- no new substance is being formed

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13
Q

Physical or Chemical: interactions between different forms of matter is

A

chemical—> produces one or more types of matter that differ from the matter before the chemical reaction

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14
Q

Physical or Chemical: interactions between matter and energy is

A

physical

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15
Q

subcategories of physical properties

A

extensive properties & intensive properties

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16
Q

phase is….

A

when you have uniform chemical properties, physically distinct, and mechanically separable

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17
Q

is cooking a protein a physical or chemical change?

A

chemical

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18
Q

Solid –> gas

A

sublimation

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19
Q

Gas –> solid

A

deposition

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20
Q

aqueous is when

A

substance is dissolved in H20

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21
Q

what is mechanical energy?

A

Kinetic Energy but for bigger objects like cars

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22
Q

what is kinetic energy? (4)

A
  • the energy or any form of energy that cannot be stored
  • The greater the speed and mass, the greater the KE
  • particles of matter posses a type of KE called mechanical energy due to their continuous motion
  • independent atoms and molecules have 3 types of mechanical energy/types of motion: vibration(back &forward motion), rotation/spinning(movement about an axis), and translation(movement from place to place).
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23
Q

Motion of Solid (6) from chart

A
  • vibration motion
  • packed in crystal formation, cant move past each other
  • STRONG intermolecular attraction between particles
  • incompressible
  • fixed shape and volume
  • weakest KE
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24
Q

Motion of Liquid (6) from chart

A
  • vibration & rotation motion
  • STILL TOUCHING EACH OTHER, not organized
  • MODERATE intermolecular attraction between particles
  • incompressible
  • fixed volume, take shape of container
  • moderate KE
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25
Q

Does it take more energy to go from solid to liquid or liquid to gas?

A

liquid to gas: bcuz it takes more effort to go from rotating to translating, than vibrating to rotating –> u are acc pulling the moecules apart

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26
Q

motion of gas (6) from chart

A

–vibration, rotation, translation motion
- NOT TOUCHING EACH OTHER, not organized
- WEAK intermolecular attraction between particles
- COMPRESSABLE
- no fixed volume of shape
- strong KE

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27
Q

what 2 factors cause phase change?

A

pressure change & temperature change

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28
Q

plasma

A

gas-like state where electrons pop off gaseous atoms to create a mixture of free electrons & cations.
- requires very high temp and low pressure to exist. –> we would not see it occur naturally on earth. matter on surface of sun=plasma

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29
Q

Triple point

A

a point at a certain pressure and temp where all 3 states of matter can exist

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30
Q

Critical point

A
  • its the end point of the water/gas line
  • you have one phase–> combination of gas and liquid = supercritical fluid
  • chemically, it is still the same substance you started off with
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31
Q

triple point of water+ice+steam

A

0.01degrees celcius & 0.8 atm (atm=atmospheric pressure)

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32
Q

supercritical fluid (SCF)

A
  • a kind of liquidy gas or gassy liquid –> not to be confused with a mixture
  • can diffuse through solids like gasses but also dissolve stuff like liquids would
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33
Q

critical point of water+steam

A

374 degrees celcius & 218 atm (atm=atmospheric pressure)

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34
Q

RMR: things travel from ______ pressure to ______ pressure

A
  • high to low
  • a perfect vacuum would have 0 atm
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35
Q

ambient &/or normal pressure is

A

1.0 atm

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36
Q

does temp depend on pressure or pressure on temp

A

temp depends on pressure

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37
Q

“normal” refers to STP which is what temp and pressure

A

1 atm & 0 degrees celcius

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38
Q

if it asks for “normal” boiling point or melting point assume

A

assume atm=1

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39
Q

STP vs SATP

A

STP= Standard Temp & Pressure:1 atm & 0 degrees celcius

SATP= Standard Ambient Temp & Pressure: 1atm & 25 degrees celcius

40
Q

Endothermic process

A

The system absorbs/gains energy from surroundings –> Temp of system increases & temp of surroundings decreases

41
Q

Exothermic process

A

The system releases/loses energy to the surroundings –> Temp of system decreases & temp of surroundings increases
- humans are constantly doing the exothermic process

42
Q

Thermal energy

A
  • KE+PE
  • is the energy contained within a system that is responsible for temp
43
Q

Heat

A

flow of thermal energy from high temp object to low temp object

44
Q

heat of fusion

A

the amount of heat required to melt a specified amount of a certain solid substance
- no change in KE, temp stays same
–> denotated with the plateau line (see page 12)

45
Q

Heat of vaporization

A

the amount of heat required to vaporize a specified amount of a certain liquid substance
- no change in KE, temp stays same

46
Q

temperature

A

average thermal energy (speed) of the molecules.

47
Q

During phase change, energy is used to

A

break or weaken the interactive forces between molecules to trigger a change in state (PE is affected)
–> all energy goes towards this and therefore KE stays constant= temp stays constant

48
Q

when energy is added, the particles will do one of 2 things

A
  • speed up –> temp increases (KE increases)
  • get pulled apart –> phase change (PE increases)
    –> never both at the same time
49
Q

As height increase atm increases or decreases

A

decreases

50
Q

the 2 ways energy is stored

A
  • thermal (due to motion of particles)
  • phase (due to attraction between particles)
51
Q

attractions increase or decrease the energy state

A
  • decreases
  • one must add energy to a system to pull particles apart
52
Q

3 ways energy is transferred/added to a system

A
  • heating (Q) –> one we look at
  • working (W)
  • radiating (R)
53
Q

the lower the energy the more _____ the object

A

stable ; therefore solids are the most stable

54
Q

difference between mixture & pure substance

A

mixture can be physically separated

55
Q

difference between compound & elements

A

compounds can be chemically decomposed

56
Q

simplest unit of matter is

A

atoms
- can exist under lab conditions

57
Q

metalloids are

A

elements intermediate in properties between metals and non-metals.
- located at staircase

58
Q

properties of metals (5)

A
  • solids @ room temp except mercury (liquid, rmr hollow letters)
  • ductile: can be stretched into thin wire
  • metallic lustre (shiny)
    -malleable: can be hammered into thin sheet
  • Good conductors of heat and electricity
59
Q

properties of metalloids (4)

A
  • Properties of both metals & non-metals
  • metallic lustre (shiny)
  • brittle: easily broken
  • semi conductors of heat and electricity
60
Q

properties of non-metals (4)

A
  • Can be solid, liquid, or gas
  • dull
  • brittle: easily broken
  • insulators
61
Q

pure substances consist of only

A

one type of substance
- can be one element or compound

62
Q

1st Group/family on periodic table

A
  • Alkali metals
63
Q

2nd Group/family on periodic table

A
  • Alkali earth metals
64
Q

3rd-12th Group/family on periodic table

A
  • Transition metals
65
Q

13th Group/family on periodic table

A
  • Boron family
66
Q

14th Group/family on periodic table

A
  • Carbon family
67
Q

15th Group/family on periodic table

A
  • nitrogen family
68
Q

16th Group/family on periodic table

A
  • oxygen family
69
Q

17th Group/family on periodic table

A
  • halogens
70
Q

18th Group/family on periodic table

A
  • noble gases
71
Q

elements 57-70 and 89-102

A
  • inner transition metals aka rare metals
72
Q

elements 57-70

A
  • Lanthanides
73
Q

elements 89-102

A
  • actinides
74
Q

Monoatomic elements

A

composed of only single atom: Cu, C

75
Q

Diatomic elements

A

2 of the same atoms bonded together: H2, O2, F2, Br2, I2, N2, Cl2

76
Q

Hydrogen is unique bcuz

A
  • non-metal but behaves like a metal
  • has some chemical properties of metals but mostly non-metals–> therefore considered non-metal
  • hydrogen is so unique that it’s usually considered to be in its own group
77
Q

Compounds have a _____ ratio

A

fixed
–> cant be changed

78
Q

Organic & inorganic compounds

A
  • organic compounds: consists of carbon and hydrogen atoms. can have other types of atoms.
  • inorganic compounds: does not have both hydrogen and carbon
79
Q

binary vs non-binary compounds

A
  • binary compound: made up with only 2 elements ex Propane C3H8
  • non-binary compound: made up of 3 or more elements ex sulfuric acid H2SO4
80
Q

Ionic compound

A
  • consists of positively charged metal ion & negatively charged non-metal ion held together by their opposite charges
  • ions are packed in CRYSTAL LATTICE arrangement. SEE page 20
81
Q

Molecular Compounds

A

consists of non-metal atoms sharing electrons

82
Q

covalent bond

A

the shared pair of valence electrons that holds 2 non-metals together

83
Q

What is a mixture?

A
  • Combination of 2 or more different substances in no fixed ratio and not bonded together –> just blended
  • substances keep their own properties and can be physically separated
84
Q

Homogenous mixture

A
  • a mixture that looks the same throughout
85
Q

Solution and its parts (4)

A
  • a homogenous mixture in which the constituent chemical species (components) do not aggregate (clump together) to form particles greater than 1 nm (1x10^9m)
    -solute: the minor component, the one being dissolved
  • solvent: the major component of the mixture, what the solute was being disolved in
  • solution is one phase, with solute evenly spread
86
Q

alloys and examples

A
  • mixture of 2 or more metals resulting in unique, desired properties
    steel: iron + chromium + carbon
    Bronze: copper+other metals:zinc or tin
    brass: zinc+other metals
87
Q

Heterogenous mixture (3)

A

mixture that doesn’t appear same throughout –> one or more component visible
- can be uniformly or non-uniformly mixed
- at least some particles greater than 1000nm or (1um=micrometer)

88
Q

Colloid (3)

A
  • seems to fall under heterogenous
  • like solution but solute particles 1nm-1000nm –> the closer to 1000nm= more behaviour like suspension, the closer to 1nm= behaviour like solution
  • appears homogenous cuz particles not large enough to settle (do not aggregate)
  • include gels, sols, emulsions –> can not be separated like suspension like filtering or centrifuging
89
Q

Suspension (4)

A
  • solute particles >1000nm or 1um
  • has a dispersed phase and a continuous medium. –> Dispersed phase: solute, Dispersed medium: solvent
  • sediment: the large particles that settle when left undisturbed
  • ex, shake before use products
90
Q

Tyndall effect is

A

is the scattering of light by a medium containing small suspended(dispersed) particles

91
Q

Tyndall effect for solutions

A
  • light not visible through solution as solute particles are too small to reflect and scatter light
92
Q

Tyndall effect for colloids

A
  • light are visible through colloid as solute particles reflect and consequently reflect light in all directions, including into your eyes
93
Q

Tyndall effect for suspension

A
  • light not visible through solution as solute particles settle, and solvent particles too small
  • to see light, either lower light source to bottom where particles settle or stir the suspension to evenly disperse the solute particles
94
Q

methods of mixture separation

A
  • components of mixture can be separated by mechanical means: picking, sifting, shaking, spinning, pouring, skimming
  • Transparency test: solution & colloid transparent to diff degrees
  • Filtration test: solutions not filtrable, colloids mostly not filtrable but large particles can be filtered by ultra-filtration, suspension components can be separated by ordinary filtration
  • centifugation: using centripetal orbit to cause large particles to settle. the liquid can be decanted (poured off)
95
Q

Particle type , properties, appearance, separation of solutions, colloids, and suspensions

A

PARTICLE TYPE
Solution: ions, atoms, small molecules
Colloid: large molecules or particles
Suspension: large particles or aggregates
PROPERTIES
Solution: Solute takes properties of solvent
Colloid & Suspension: immediate properties of solute and solvent
APPEARANCE
Solution: clear
Colloid & Suspension: cloudy
SEPARATION
Solution & Colloid: do not separate
Suspension: Separate to form sediment

Chemistry (8 decks)

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