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Chemistry SOL > Chemistry SOL Vocab and Formula's > Flashcards

Chemistry SOL Vocab and Formula's Flashcards

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0
Q

Density Formula

A

Density = Mass
______
Volume

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1
Q

Percent Error

A

True - Observed x 100
_____________________ (error is
True absolute so it Cannot be negative)

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2
Q

Percent Yield

A

Observed x 100
_________
True

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3
Q

Independent Variable

A

The variable that the experimenter plans to change

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4
Q

Dependent Variable

A

What changes as a result of the experiment

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5
Q

Control

A

The standard that is used for comparison

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6
Q

Constants

A

The parts of the experiment that do not vary

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7
Q

Molarity formula

A

Molarity (M) = Moles of solute
_______________
Liters of solution

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8
Q

Accuracy

A

How close to True Value

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9
Q

Precision

A

Getting the same outcome over and over again

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10
Q

Reliability

A

Using the same tools/equipment every time

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11
Q

(Significant Digits) Leading 0

A

Never Significant

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12
Q

Sandwich 0

A

Always significant

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13
Q

Trailing 0

A

Only if decimal in problem

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14
Q

Add or Subtract

A

Lowest # of decimal places

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15
Q

Multiply or Divide

A

Lowest # of Sig Digits

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16
Q

Basic Units of Measurement :

Length
Volume
Mass
Temperature
Time
A

Length - meters (m)

Volume - milliliters (mL) or cubic centimeters (cm^3)

Mass - Grams (g)

Temperature = degrees Celsius (C) or Kelvin (K)

Time = seconds (s)

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17
Q

Prefixes (Milli, Centi, Deci, Kilo)

A

Milli - 1/1000

Centi - 1/100

Deci - 1/10

Kilo - 1000

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18
Q

Dalton

A

Father of the modern atomic atomic theory - thought atom looked like a solid sphere

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19
Q

Thomson

A

Cathode Ray Tube experiment - Proved that electrons, smaller particles than atoms, exist - led to plum pudding model of atom where charged are scattered all over atom

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20
Q

Milikan

A

Oil Drop Experiment - Discovered mass and charge of electron

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21
Q

Rutherford

A

Gold Foil Experiment - Determined that atoms are mostly empty space with small, dense nucleus at the center

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22
Q

Bohr

A

Planetary model of atom where electrons orbit nucleus in energy levels

                                            OR

Electrons occupy an energy level

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23
Q

The Quantum Mechanical Model

A

Model of the atom that we us today

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24
Q

Planck

A

Matter can gain or lose energy in small specific amounts = Quantum Theory of Energy

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25
Q

de Broglie

A

Electrons act as both waves and particles

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26
Q

Heisenburg

A

Uncertainty Principle - Can’t predict both speed and location of electron at the same time because they act like both particles and waves

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27
Q

Isotope

A

Same number of protons but different number of neutrons

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28
Q

Ion

A

Same number of protons but different number of electrons

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29
Q

Half life

A

The amount of time for half the atoms in a sample to decay

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30
Q

Fission

A

Splitting atoms, releases neutrons, makes heat

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31
Q

Fusion

A

Putting together small atoms to make bigger ones, makes lots of heat (the sun)

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32
Q

Alpha Particle (Mass, Charge, And Composition, Shielding)

A

Mass: 4
Charge: +2
Composition: 2P + 2N
Shielding: Paper/ skin

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33
Q

Beta

A

Mass: 0
Charge: -1
Composition: Electron
Shielding: Few sheets of aluminum foil

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34
Q

Gamma

A

Mass: 0
Charge: 0
Composition: Energy
Shielding: Concrete or several cm of lead

35
Q

When balancing nuclear equations, what two properties must be conserved

A

Mass and Charge

36
Q

Aufbau Principle

A

Electrons go in lowest energy level and sub level first

37
Q

Hund’s Rule

A

Each orbital in a sub level must be full before doubling up

38
Q

Pauli Exclusion Principle

A

The two electrons in each orbital have opposite spins

39
Q

Atomic Radius

A

Distance from nucleus to valence electrons (biggest = Francium)

40
Q

Electronegativity

A

Ability of atom to attract electrons from another atom

most electrongativity = Fluorine

41
Q

Ionization Energy

A

Energy required to remove an electron from an atom

most ionization energy = Helium

42
Q

Metal Reactivity

A

(most reactive metal = Francium)

43
Q

NonMetal Reactivity

A

(Most reactive Nonmetal = Fluorine)

44
Q

Ionic Compound

A

Metal + Nonmetal; Transfer electrons; soluble in water, conductors, high melting point

45
Q

Covalent/Molecular compound

A

Nonmetal + Nonmetal; share electrons; insoluble in water, non conductors, low melting point.

46
Q

Alcohol

A

-OH

47
Q

Ether

A

-O-

48
Q

Carboxylic Acid

A

-C-OH

49
Q

Ketone

A

-C-

50
Q

Ester

A

-C-O-

51
Q

Aldehyde

A

-C-H

52
Q

Amine

A

-NH2

53
Q

Amide

A

-C-NH2

54
Q

STP

A

0 C = 273K

1atm = 760torr = 760mmHg = 101.3kPa

55
Q

(Gas Laws) Boyle’s Law

A

Inverse relationship between Pressure and Volume

56
Q

Charles’ Law

A

Direct Relationship between Volume and Temperature (V/T)

57
Q

Gay-Lussac’s Law

A

Direct Relationship between Pressure and Temperature (P/T)

58
Q

Dalton’s Law of Partial Pressure

A

Ptotal = P1 + P2 + P3….

59
Q

Hydrochloric Acid

A

HCl

60
Q

Sulfuric Acid

A

H2SO4

61
Q

Nitric Acid

A

HNO3

62
Q

Phosphoric Acid

A

H3PO4

63
Q

Acids

A

pH less than 7

64
Q

Bases

A

pH more than 7

65
Q

Triple point

A

Place where all 3 phases coexist

66
Q

Critical Point

A

Temperature where only gas phase exist

67
Q

Diatomic Molecules

A

Br2 I2 N2 Cl2 H2 O2 F2

Brinclhof

68
Q

Proton (Mass, Charge, Location)

A

Mass: 1 amu
Charge: +1
Location: Nucleus

69
Q

Neutron (Mass, Charge, Location)

A

Mass: 1 amu
Charge: 0
Location: Nucleus

70
Q

Electron (Mass, charge, and Location)

A

Mass: 0 amu
Charge: -1
Location: Energy Levels

71
Q

Two Main Aspects of an Atom are the

A

Nucleus and energy Levels

72
Q

An Electron dot diagram consist of what two things?

A

Element Symbol + Valance electrons represented by dots

73
Q

In isotopic notation of atoms the number in the upper left refers to the ____________ and the number in the lower left refers to __________

14 C
6

A

1: Atomic Mass
2: Number of Protons

74
Q

How would a electron become more stable?

A

The closer it is to the nucleus the more stable it becomes

75
Q

Six ways to separate a mixture

A

Filtration

Evaporation

Distillation

Decanting

Chromatography

Centrifuging

76
Q

Filtration

A

Separating out by size of Particles

77
Q

Evaporation

A

Separation by phase change (Liquid + Solid)

78
Q

Distillation

A

Separation based on boiling point (Liquid + Liquid)

79
Q

Decanting

A

Pouring

80
Q

Chromatography

A

Separating pigments

81
Q

Centrifuging

A

Separation by spinning (Separates by density)

82
Q

Physical Property

A

an aspect of matter that can be observed or measured without changing it

83
Q

Chemical Property

A

An aspect of matter that can be observed by the chemical identity of a substance

84
Q

Physical Change

A

You can get the substance back

85
Q

Chemical Change

A

You can’t get the substance Back

86
Q

Hydrogen gas is a combination of what

A

Acid + Metal

Chemistry SOL (2 decks)

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