Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry Final Review > Tri 1 > Flashcards

Tri 1 Flashcards

(100 cards)

Start Studying
1
Q

What is accuracy?

A

How close the measured value is to the actual quantity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is precision?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Celsius to Kelvin?

A

+273

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Kelvin to Celsius?

A

-273

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Addition and subtraction operations

A

Count decimal places, the fewest one

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Multiplication and division operations

A

Count number of significant figures, fewest one

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Democritus

A

“Átomos” Concept of atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Antoine Lavoisier

A

Law of conservation of mass (LAV LAW)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

John Dalton

A

1st atomic theory, water is always H20

-4 postulates

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Joseph Proust

A

The law of definite proportions (PROUST PROPORTIONS)

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

JJ Thompson

A

Cathode ray tube. Electrons are negative

THOMPSON TUBE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Earnest Rutherford

A

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

rutherFORD FOIL

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Max Planck

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Albert Einstein

A

A beam of light is a stream of particles called photons

EINSTEIN PHOTON

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Atomic number

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Mass number

A

Neutrons + protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Average atomic mass

A

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

% into decimal!

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Planck equation

A

E=hv

E= energy per quantum
H= plancks constant (6.63x10^-34)
V= frequency
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Orbitals

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Atomic radius

A

Decreases↗️

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Ionization energy

A

Increases↗️⬆️➡️

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Electronegativity

A

An elements ability to attract electrons in a chemical bond.

Increase↗️➡️⬆️

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Ions

A

Element with a different charge.
Metals +
Non metals -

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Binary Covalent Compounds
2 non metals PREFIXES
26
Prefixes
Mono, di, tri, tetra, penta, hexa, hepta, Octa, Nona, deca
27
Covalent compounds
The second one turns to ide
28
Polyatomic ions
Ends in ide, ate, ite
29
Acids
Ate to ic Ite to ous NO OXYGEN: SAY HYDRO OXYGEN: DONT SAY HYDRO
30
LiCl
Lithium Chloride
31
FeO
Iron (ll) Oxide
32
AgNO3
Silver nitrate
33
Zinc Chloride
ZnCl2
34
Tin (ll) Chloride
SnCl2
35
CO
Carbon monoxide
36
N20
Dinitrogen monoxide
37
CCl4
Carbon tetrachloride
38
Disulfur dichloride
S2Cl2
39
Lead (ll) Nitrate
Pb(Ni)2
40
Silver Cyanide
AgCN
41
HCl
Hydrochloric acid
42
Hydrobromic acid
HBr
43
H2SO3
Sulfurous acid
44
Carbonic Acid
H2CO3
45
Stoichiometry
Convert to moles Ratio Convert back to grams
46
Limiting reactant
The reactant that is used up limits how far the reaction will proceed
47
Avogadro’s number
Used to find amount of molecules in a mole 6.022 x 10^23 mol
48
Mass percent
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
Molecular formula
Actual formula Molar mass —
50
Empirical formula
Ratio in simplest form
51
Octet rule
Elements gain lose or share electrons to acquire a full octet
52
Non metals
Always gain electrons (more negative)
53
Metals
Lose electrons. Always positive
54
Ionic bonding
Metals and non metals bond. Metals transfer electrons
55
Melting point of ionic solids
Larger distance (bigger radius) = weaker bond Shorter distance= stronger bond
56
Covalent bonds
Sharing electrons (2 NON METALS)
57
Polyatomic ions
2 Non metals Or A metal and a non metal
58
Lewis Structures
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
Linear
2 charge clouds and 2 bonds 5 charge clouds, 2 bonds, 3 lone pairs
60
Trigonal planar
3 charge clouds and 3 bonds
61
Bent
3 charge clouds, 2 bonds, 1 lone pair 4 charge clouds, 2 bonds, 2 lone pairs
62
Tetrahedral
4 charge clouds and 4 bonds
63
Trigonal pyramidal
4 charge clouds, 3 bonds, 1 lone pair
64
Trigonal bipyramidal
5 charge clouds, 5 bonds
65
Seesaw
5 charge clouds, 4 bonds, 1 lone pair
66
T-shaped
5 charge clouds, 3 bonds, 2 lone pairs
67
Octahedral
6 charge clouds, 6 bonds
68
Octahedral
6 charge clouds, 5 bonds, 1 lone pair
69
Square planar
6 charge clouds, 4 bonds, 2 lone pairs
70
Hybrid orbitals
``` 2 charge clouds- sp 3 charge clouds- sp2 4 charge clouds- sp3 5 charge clouds- sp3d 6 charge clouds-sp3d2 ```
71
Formal charge
Formal charge = the number of valence electrons assigned to neutral atom - the number of electrons assigned to the atom in the structure
72
Bond order
Number of bonds
73
Sigma bond
Single bond
74
Pi bond
Double bond
75
OXIDIZE
LOSES ELECTRONS (MORE POSITIVE)
76
REDUCE
GAINS ELECTRONS (MORE NEGATIVE)
77
Solvent
The substance you have more of
78
Solute
The substance you have less of
79
Solubility rules
Na+, K+, NH4+, NO3-, C2H3O2- are soluble in water
80
Double replacement (non redox)
Two things switch AB+CD➡️AD+CB Precipitation
81
Combustion (redox)
Hydrocarbon + O2➡️CO2 + H2O
82
Single replacement (redox)
Metal-metal Metal-hydrogen Non metal- non metal (halogens) A+BC➡️B+AC
83
Synthesis/decomposition (redox)
A+B➡️AB CD➡️C+D
84
Ox
Zn➡️Zn+2 + 2 e-
85
Red
Cu+2 + 2 e-➡️Cu
86
Half reactions (ACIDS)
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
Nitrate in acid
NO3-➡️NO
88
Permanganate in acid
MnO4-➡️Mn2+
89
Dichromate in acid
Cr2O7-2➡️Cr3-
90
Oxidation of sulfite
SO32-➡️SO42-
91
Oxidation of hydrogen peroxide
H2O2➡️O2
92
Metals will always be....
Oxidized!
93
Exothermic
Feels hot! Energy exiting
94
Endothermic
Feel cold! Heat goes from hot to cold so the heat from your hand is ENTERING the system
95
🔺H
Enthalpy Change ( change in heat)
96
🔺H equation
🔺H= sum of bonds broken-sum of bonds formed
97
🔺S
Entropy | Amount of disorder.
98
🔺S equation
🔺S= S products - S reactants
99
Gibbs Free Energy
🔺G= 🔺H-T(🔺S) IF G IS NEGATIVE, THE RXN IS FAVORED
100
Delta G
THE G HAS TO BE NEGATIVE FOR IT TO BE FAVORED!!!!

Chemistry Final Review (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions