Unit A: Sections 1&2 (Grade 8) Flashcards

Most questions in this deck relate mainly to the following: - Matter (particles, Kinetic Energy...) - Safety in the Lab (WHMIS, Hazard Symbols, etc)

1
Q

Particle Model of Matter

A

PMAST
All matter is made of tiny PARTICLES.
The particles are always MOVING or VIBRATING (have kinetic energy).
The particles are ATTRACTED to each other and have SPACES between them.
As TEMPERATURE increases, the particles move more (kinetic energy increases)

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2
Q

Hazard Symbol

A

A sign that tells you to be aware and careful while handling said substance.
Shape/Colour indicates HOW dangerous something is
The symbol tells you WHAT the danger is.
- More sides = More danger
- Yellow - Red = Increasing in danger

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3
Q

WHMIS

A

Workplace
Hazardous
Materials
Information
System

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4
Q

Fluids

What are fluids? What are their properties?

A

Can be liquids or gases
Anything that has no fixed shape and can flow
1. Move Materials (Hose washing mud)
2. Process Materials
- Glass - shape comes from melting into liquid
- Steel - when mixture of elements melted together,
forms a solid
3. Use Materials (Toothpaste - a fluid - HOLDS tooth detergents)

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5
Q

Slurries

A

Mixtures of water and solids (mud/dirt)

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6
Q

Matter

What is Matter?

A
  • Anything that takes up space
  • Made up of tiny particles invisible to the naked eye
  • Has mass
  • physicaly separated between pure substances and mixtures
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7
Q

Metal

A

A substance that conducts electricity
[Does it conduct electricity?]
[Yes –> Metal]
[No –> Non-Metal]

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8
Q

Sublimation

A

Solid-Gas

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9
Q

Deposition

A

Gas-Solid

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10
Q

Pure Substance

A
  • Made up of one type of particle that cannot be separated
  • All particles of one pure substance that is all the same
  • Can be [chemical reactions are] elements or compounds
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11
Q

Mixtures

A

Multiple substances mixed
Can be classified as either homogeneous (solution) or heterogeneous
Has 3 heter. types
- Mechanical Mixture
- Suspension
- Colloid

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12
Q

Homogeneous

Provide example(s)

A

Looks like 1 substance (coffee, tea)

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13
Q

Heterogeneous

A

Can see all different parts (pizza, cookie, cereal)

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14
Q

Compound

A

A substance that consists of multiple elements

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14
Q

Element

A

Something that cannot be simplified/broken down into simpler substances by chemical means

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15
Q

Mechanical Mixture

Provide Examples

A

Can be identified and disassembled (cookie, chili, stew)

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16
Q

Suspension

Provide Example

A

Cloudy mixture in which droplets are suspended in another substance (oil in water)

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17
Q

Colloid

A

Cloudy mixtures, but the droplets are so small that they don’t separate easily (milk)

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18
Q

Solution

Howdo you get a solution? What is it?

A
  • Particles of one “fit” between others, making it look like one substance
  • A homogenous mixture
  • Multiple pure substances mixed
    Dissolving one substance into another = Solution
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19
Q

mPhysical Properties

A
  • Can be OBSERVED/MEASURED without altering the substance
  • Observable with 5 senses
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20
Q

Physical Changes

A

The substance (CHEMICAL MAKEUP) is not changed.
Size
State
Form

(Water/Ripping Paper)

21
Q

Qualitative

A

Only requires observations and descriptors ((colour, viscosity, lustre, texture, etc.))

22
Q

Quantitative

A

Properties that can be measured ((boiling/melting point, electrical conductivity, density, viscosity))

23
Q

Chemical Changes

A

When multiple substances combine to create a new/verydifferent substance.
Chemical changes are changes in colour, odour, formation of gas/solids, release/absorption of heat

24
Chemical Properties
Describes how a substance interacts with another. Chemical properties include reactions with Acids, Water, Heat, Burns, Oxygen/Air
25
Endothermic
Absorption of heat. (En=Enter) Feels COLD
26
Exothermic
Release of heat. (Ex=Exit) Feels HOT
27
Solute
The substance that dissolves within another substance (sugar)
28
Solvent
The substance that does the dissolving (water)
29
Concentrated // (-tion)
A solution with LOTS of solute compared to the solvent Amount of solute within the solvent Solute/Solvent x 100% g/mL x 100%
30
Dilute
A solution with LITTLE solute compared to solvent (whiskey and water)
31
Solubility
The MAXIMUM amount of solute that can be dissolved within the solvent at a given TEMPERATURE. Solute/Temperature x 100%
32
Saturation Point
The point where no more solute can be added to the solvent; the solvent/solution resists.
33
PPE
Personal Protective Equipment
34
Saturated
A saturated solution is a solution in which no more solute can dissolve at a given temperature Value = On Line
35
Unsaturated
More solute can dissolve Value = Below Line
36
Supersaturated
A supersaturated solution is one that contains more solute than it normally would be able to dissolve at a certain temperature
37
What affects the dissolving rate in solutions?
Agitation - shaking/stirring Temperature - increasing speeds, decreasing slows Surface Area - solution takes up more space (wide)
38
What does water weigh?
1 g/mL
39
Properties
Characteristics that describe matter
40
Lustre
Shine
41
Hardness
A substance's ability to resist being scratched Can be measured by the Mohs' Scale Talc-Diamond
42
Melting Point (PHP)
The point where subs. changes from solid-liquid (Water = 0°C)
43
Boiling point (PHP)
The temperature at which a subs. changes from liquid-gas (Water = 100°C)
44
Malleability
The ability to be compressed/folded into sheets (aluminum)
45
Ductility
Ability to be stretched into long wires (copper)
46
Density
Amount of mass in a given volume of a subs. Water = 1g/mL
47
Conductivity
Ability to conduct electricity or heat (think conductors and insulators)
48
Plasticity
Can be shaped/molded
49
Crystal
A substance having a distinct shape for crystal Silicon crystals are diamond-shaped, and salt is in cubes