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Chemistry Final Review > Tri 1 > Flashcards

Tri 1 Flashcards

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1
Q

What is accuracy?

A

How close the measured value is to the actual quantity

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2
Q

What is precision?

A

How close 2 or more measurements of the same quantity are to one another

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3
Q

Celsius to Kelvin?

A

+273

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4
Q

Kelvin to Celsius?

A

-273

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5
Q

Addition and subtraction operations

A

Count decimal places, the fewest one

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6
Q

Multiplication and division operations

A

Count number of significant figures, fewest one

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7
Q

Democritus

A

“Átomos” Concept of atoms

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8
Q

Antoine Lavoisier

A

Law of conservation of mass (LAV LAW)

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9
Q

John Dalton

A

1st atomic theory, water is always H20

-4 postulates

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10
Q

Joseph Proust

A

The law of definite proportions (PROUST PROPORTIONS)

Ex. Water is always 88% oxygen and 11% hydrogen

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11
Q

JJ Thompson

A

Cathode ray tube. Electrons are negative

THOMPSON TUBE

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12
Q

Earnest Rutherford

A

Gold foil. Atoms have a nucleus. Protons are positive.

rutherFORD FOIL

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13
Q

What is an isotope?

A

Same element. DIFFERENT NUMBER OF NEUTRONS.

Exhibit identical chemical behavior
Mass number is the same but atomic number stays the same

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14
Q

Max Planck

A

Quantum theory and Planck’s constant
(PLANCK QUANTUM)
-energy radiates from a heated object

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15
Q

Albert Einstein

A

A beam of light is a stream of particles called photons

EINSTEIN PHOTON

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16
Q

Atomic number

A

The number of protons (or electrons in a neutral atom )

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17
Q

Mass number

A

Neutrons + protons

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18
Q

Average atomic mass

A

(Mass# x %)+(Mass# x %) = average atomic mass

% into decimal!

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19
Q

Planck equation

A

E=hv

E= energy per quantum
H= plancks constant (6.63x10^-34)
V= frequency
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20
Q

Orbitals

A

1s,2s,2p,3s,3p,3d,4s,4p,4d,4f,5s,5p,5d

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21
Q

Atomic radius

A

Decreases↗️

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22
Q

Ionization energy

A

Increases↗️⬆️➡️

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23
Q

Electronegativity

A

An elements ability to attract electrons in a chemical bond.

Increase↗️➡️⬆️

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24
Q

Ions

A

Element with a different charge.
Metals +
Non metals -

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25
Q

Binary Covalent Compounds

A

2 non metals PREFIXES

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26
Q

Prefixes

A

Mono, di, tri, tetra, penta, hexa, hepta, Octa, Nona, deca

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27
Q

Covalent compounds

A

The second one turns to ide

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28
Q

Polyatomic ions

A

Ends in ide, ate, ite

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29
Q

Acids

A

Ate to ic
Ite to ous

NO OXYGEN: SAY HYDRO
OXYGEN: DONT SAY HYDRO

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30
Q

LiCl

A

Lithium Chloride

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31
Q

FeO

A

Iron (ll) Oxide

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32
Q

AgNO3

A

Silver nitrate

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33
Q

Zinc Chloride

A

ZnCl2

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34
Q

Tin (ll) Chloride

A

SnCl2

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35
Q

CO

A

Carbon monoxide

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36
Q

N20

A

Dinitrogen monoxide

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37
Q

CCl4

A

Carbon tetrachloride

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38
Q

Disulfur dichloride

A

S2Cl2

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39
Q

Lead (ll) Nitrate

A

Pb(Ni)2

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40
Q

Silver Cyanide

A

AgCN

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41
Q

HCl

A

Hydrochloric acid

42
Q

Hydrobromic acid

A

HBr

43
Q

H2SO3

A

Sulfurous acid

44
Q

Carbonic Acid

A

H2CO3

45
Q

Stoichiometry

A

Convert to moles
Ratio
Convert back to grams

46
Q

Limiting reactant

A

The reactant that is used up limits how far the reaction will proceed

47
Q

Avogadro’s number

A

Used to find amount of molecules in a mole

6.022 x 10^23 mol

48
Q

Mass percent

A

The percentage by mass of an element in a compound or a component in a substance

Mass% element = (# of atoms in element)(elements atomic mass) x 100/ formula weight of compound

49
Q

Molecular formula

A

Actual formula

Molar mass
—

50
Q

Empirical formula

A

Ratio in simplest form

51
Q

Octet rule

A

Elements gain lose or share electrons to acquire a full octet

52
Q

Non metals

A

Always gain electrons (more negative)

53
Q

Metals

A

Lose electrons. Always positive

54
Q

Ionic bonding

A

Metals and non metals bond. Metals transfer electrons

55
Q

Melting point of ionic solids

A

Larger distance (bigger radius) = weaker bond

Shorter distance= stronger bond

56
Q

Covalent bonds

A

Sharing electrons (2 NON METALS)

57
Q

Polyatomic ions

A

2 Non metals

Or

A metal and a non metal

58
Q

Lewis Structures

A
  1. Count the total number of valence electrons in the molecule
  2. Put the least electronegative in Center and connect terminal atoms to it with single bonds. -
  3. Complete octet for all terminal atoms except for H
  4. Add electrons used and subtract from valence electrons, attach leftover electrons to the central atom as lone pairs
  5. Make multiple bonds to complete Central atom octet
59
Q

Linear

A

2 charge clouds and 2 bonds

5 charge clouds, 2 bonds, 3 lone pairs

60
Q

Trigonal planar

A

3 charge clouds and 3 bonds

61
Q

Bent

A

3 charge clouds, 2 bonds, 1 lone pair

4 charge clouds, 2 bonds, 2 lone pairs

62
Q

Tetrahedral

A

4 charge clouds and 4 bonds

63
Q

Trigonal pyramidal

A

4 charge clouds, 3 bonds, 1 lone pair

64
Q

Trigonal bipyramidal

A

5 charge clouds, 5 bonds

65
Q

Seesaw

A

5 charge clouds, 4 bonds, 1 lone pair

66
Q

T-shaped

A

5 charge clouds, 3 bonds, 2 lone pairs

67
Q

Octahedral

A

6 charge clouds, 6 bonds

68
Q

Octahedral

A

6 charge clouds, 5 bonds, 1 lone pair

69
Q

Square planar

A

6 charge clouds, 4 bonds, 2 lone pairs

70
Q

Hybrid orbitals

A 
2 charge clouds- sp
3 charge clouds- sp2
4 charge clouds- sp3
5 charge clouds- sp3d
6 charge clouds-sp3d2
71
Q

Formal charge

A

Formal charge = the number of valence electrons assigned to neutral atom - the number of electrons assigned to the atom in the structure

72
Q

Bond order

A

Number of bonds

73
Q

Sigma bond

A

Single bond

74
Q

Pi bond

A

Double bond

75
Q

OXIDIZE

A

LOSES ELECTRONS (MORE POSITIVE)

76
Q

REDUCE

A

GAINS ELECTRONS (MORE NEGATIVE)

77
Q

Solvent

A

The substance you have more of

78
Q

Solute

A

The substance you have less of

79
Q

Solubility rules

A

Na+, K+, NH4+, NO3-, C2H3O2- are soluble in water

80
Q

Double replacement (non redox)

A

Two things switch
AB+CD➡️AD+CB
Precipitation

81
Q

Combustion (redox)

A

Hydrocarbon + O2➡️CO2 + H2O

82
Q

Single replacement (redox)

A

Metal-metal

Metal-hydrogen

Non metal- non metal (halogens)

A+BC➡️B+AC

83
Q

Synthesis/decomposition (redox)

A

A+B➡️AB

CD➡️C+D

84
Q

Ox

A

Zn➡️Zn+2 + 2 e-

85
Q

Red

A

Cu+2 + 2 e-➡️Cu

86
Q

Half reactions (ACIDS)

A
  1. Balance atoms except for O and H
  2. Balance O by adding H2O
  3. Balance H by adding H+
  4. Balance charge by adding electrons
  5. Cross multiply to cancel electrons
  6. Add half reactions and cancel things that are the same
87
Q

Nitrate in acid

A

NO3-➡️NO

88
Q

Permanganate in acid

A

MnO4-➡️Mn2+

89
Q

Dichromate in acid

A

Cr2O7-2➡️Cr3-

90
Q

Oxidation of sulfite

A

SO32-➡️SO42-

91
Q

Oxidation of hydrogen peroxide

A

H2O2➡️O2

92
Q

Metals will always be….

A

Oxidized!

93
Q

Exothermic

A

Feels hot! Energy exiting

94
Q

Endothermic

A

Feel cold! Heat goes from hot to cold so the heat from your hand is ENTERING the system

95
Q

🔺H

A

Enthalpy Change ( change in heat)

96
Q

🔺H equation

A

🔺H= sum of bonds broken-sum of bonds formed

97
Q

🔺S

A

Entropy

Amount of disorder.

98
Q

🔺S equation

A

🔺S= S products - S reactants

99
Q

Gibbs Free Energy

A

🔺G= 🔺H-T(🔺S)

IF G IS NEGATIVE, THE RXN IS FAVORED

100
Q

Delta G

A

THE G HAS TO BE NEGATIVE FOR IT TO BE FAVORED!!!!

Chemistry Final Review (1 decks)

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