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#! Flashcards

1
Q

Properties of a Solid : (Shape, Volume, Expansion, Compressibility)

A

Incompressible, Compressible, Slight, Almost Cannot

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2
Q

Properties of a Liquid : (Shape, Volume, Expansion, Compressibility)

A

Compressible, Incompressible, Moderate, Almost Cannot

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3
Q

Properties of a Gas/Vapor : (Shape, Volume, Expansion, Compressibility)

A

Compressible, Compressible, Great, Almost Can

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4
Q

State the 6 Phase Changes

A

Melting, Freezing, Condensation, Vaporization, Sublimation, Deposition

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5
Q

What is Melting (is energy released or taken in?)

A

Solid to Liquid (Take in energy) Fusion*

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6
Q

What is Freezing (is energy released or taken in?)

A

Liquid to Solid (Release energy) Solidification and Crystallization*

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7
Q

What is Condensation (is energy released or taken in?)

A

Gas to Liquid (Release energy)

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8
Q

What is Vaporization (is energy released or taken in?)

A

Liquid to Gas (Take in energy)
Also known as boiling or evaporation

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9
Q

What is Deposition? (Is energy released or taken in?)

A

Gas to Solid (Releases Energy)

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9
Q

What is Sublimation? (Is energy released or taken in?)

A

Solid to Gas (Take in energy)

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10
Q

What are Physical Properties?

A
  • Characteristics that can be observed without changing the substance’s chemical identity.
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11
Q

What are all the Physical Properties?

A

Color, Odor, Melting Point, Boiling Point, Density (C.O.M.B.D)

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12
Q

What are Chemical Properties?

A

-Describes a substance’s ability to undergo changes that transform it into different substances.

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13
Q

What are all the Chemical Properties?

A

Flammability, Oxidation State, Reactivity (F.O.R.)

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14
Q

What are Pure Substances?

A

: Consists of only one type of atom or molecule. They are characterized by having uniform and definite composition.

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15
Q

What are the types of Pure Substances

A

Elements & Compounds

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16
Q

Give an example of a pure element

A

Carbon (C) or Gold (Au)

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17
Q

Pure: Elements

A

The pure substance only made up of only one kind of atom

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18
Q

Pure: Compounds

A

2 or more elements chemically bonded together in a fixed ratio. Always in that specific combined ratio

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19
Q

How can compounds be broken down?

A

Through Chemical Reactions

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20
Q

Give an example of a pure compound

A

Water (H20) and Carbon Dioxide (CO2)

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21
Q

What is a mixture?

A
  • 2 or more substances physically combined but not chemically bonded. Each retains its chemical property and identity.
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22
Q

What are the types of mixtures?

A

Homogeneous mixtures & Heterogeneous mixtures

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23
Q

Define Homogeneous Mixtures

A
  • Have a uniform composition throughout. (Solutions)
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24
Explain the components of a Homogenous mixture.
Components are evenly distributed and cannot be distinguished from one another.
25
Give an example of Homogenous mixtures.
Coffee, Wine, Air, Brass, Steel, Natural Gas, Vinegar, Blood
26
What can differentiate Homogenous mixtures from Heterogenous mixtures?
You cant visually distinguish the substances
27
Why is Air Homogeneous?
There is a mix of 02 and N2 in the air and you can't visually tell the difference.
27
Define Heterogenous Mixtures
Mixtures that do not have a uniform composition
28
Explain the components of a Heterogeneous mixture.
The components are unevenly distributed and can typically be separated.
29
Give an example of Heterogeneous mixtures.
Chocolate Chip Cookies, Tossed Salad, Sandwich,
30
What are the types of Purity & Separation Methods?
Filtration, Distillation, Chromatography
31
What is Filtration?
Separates Solids from Liquids
32
What is Distillation?
Separates based on boiling points
33
Explain the Filtration technique.
It uses a porous barrier or filter that allows only fluid to pass through and keeps out other molecules
34
Explain the Distillation technique.
It involves boiling the liquid mixture based on the differences in their boiling points, by vaporizing the component with the lowest boiling point and then cooling it to condense it back into a liquid collected separately.
35
Define Accuracy
- Reflects true values (preciseness)
36
Define Precision
-Yield SImilar results (consistency)
37
State the Metric Prefixes:
Femto (-15), Pico (-12), Nano (-9), Micro (-6), Milli (-3), Centi (-2), Deci (-1), Base (0), Deka (1), Hecto (2), Kilo (3), Mega (6), Giga (9), Tera (12), Peta (15)
38
How do you calculate Average Atomic Mass?
Add all the percent of mass of the isotopes.
39
What is the equation for Atomic Mass
Atomic Mass = ∑(Isotope Mass×Isotopic Abundance)
40
What happens as you move from left to right on the atomic table?
The atomic radius decreases because of the increased nuclear charge (more protons) that pulls electrons closer to the nucleus
41
What happens as you move from up to down on the atomic table?
Since additional electron shells are added, more electrons are placed farther from the nucleus.
42
What are Cations?
Positive ions
43
Compare Cations to an atom
They are smaller because they lose outer shell electrons reducing repulsion (+)
44
What are anions?
Negatively charged Ions
45
Compare Anions to an atom
They are larger because they gain electrons causing them to expand their "size"
46
H1
Protium
47
H2
Deuterium
48
H3
Tritium
49
What element is Na and what is it's Latin name
Sodium Natrium
50
Extensive Properties
Physical properties depend on the amount of matter rather than the type.
51
Intensive Properties
Physical Properties depend on the type rather than the amount
52
What element is K and what is its Latin name
Kalium Kalium
53
What element is Sb and what is its Latin name
Antimony Stibium
54
What element is Cu and what is its Latin name
Copper Cuprum
55
What element is Au and what is its Latin name
Gold Aurum
56
What element is Ag and what is its Latin name
Silver Argentum
57
What element is Fe and what is its Latin name
Iron Ferrum
58
What element is Pb and what is its Latin name
Lead Plumbum
59
What element is Hg and what is its Latin name
Mercery *Hydrargyrum*
60
What element is Sn and what is it's Latin name
Tin Stannum
61
What element is W and what is its Latin name
Tungsten Wolfram
62
Give examples of Chemical change
Chemical properties are observed only when an object undergoes a chemical change such as Burn, rot, rust, decompose, ferment, explode, and corrode.
63
What happens to energy during a chemical reaction?
The energy was lost or gained (not destroyed)
64
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Chem test Review #1 (1 decks)

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