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AP Chemistry > Chapter 1+2+3 > Flashcards

Chapter 1+2+3 Flashcards

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1
Q

Law

A

Summarizes what happens

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2
Q

Theory/model

A

Provides an explanation

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3
Q

Filtration

A

Separates insoluble solid from liquid or solution

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4
Q

Distillation

A

Uses different boiling points to separate mixtures

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5
Q

Crystallization

A

Separates using differences in solubility

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6
Q

Chromatography

A

Separates using differences in polarity

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7
Q

Extraction

A
  • Separates using differences in polarity

- Emerge both in a solvent that one dissolves into and the other does not

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8
Q

Kelvin

A

K = C + 273

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9
Q

Fahrenheit

A

F = 1.8C +32

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10
Q

Centimeter

A

M x 10^-2

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11
Q

Millimeter

A

M x 10^-3

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12
Q

Micrometer

A

M x 10^-6

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13
Q

Nanometer

A

M x 10^-9

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14
Q

Dalton’s Early Atomic Theory

A

1) Elements are composed of tiny particles called atoms
2) Atoms of the same element are exactly alike and have same properties
3) Atoms of an element can’t be created or destroyed
4) Compounds are formed when atoms of two or more elements are chemically combined in a fixed small whole number ratio

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15
Q

Law of Conservation of Mass

A

During a chemical reaction there is no detectable change between the total mass of the reactants and the mass of the products

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16
Q

Law of Constant Composition

A

A compound is always composed of the same elements in the same ratio (percentage) by mass

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17
Q

Law of Multiple Proportions

A

When two elements from more than one compound and the mass of one of the elements in each compound is held constant at 1.0 g, then the masses of the second element will be found to occur in an exact ratio of small whole numbers to each other

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18
Q

J.J. Thomson

A

Cathode Ray Tube Experiments

  • Electrons exist
  • Plum Pudding Model (picture a circle with lots of negatives floating around inside)
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19
Q

R. Millikan

A

Oil Drop Experiment

-Found charge of an electron

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20
Q

Henri Becquerel

A
  • Found that a mineral containing uranium produced its image on a photographic plate in the absence of light
  • Termed this spontaneous emission radioactivity
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21
Q

E. Rutherford

A

Gold Foil Experiment:

  • Atom is mostly empty space
  • Nucleus positively charged, small
  • Disproved Thomson’s plum pudding

Three types of radiation: Alpha, Beta, Gamma
Alpha: 4 mass, +2 charge
Beta: Basically no mass, -1 charge
Gamma: 0 mass, 0 charge

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22
Q

J. Balmer

A

Visible Light Emission Spectra Experiments

  • Elements have unique spectral lines
  • Each line was determined to represent an electron energy “jump” between energy levels
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23
Q

H. Moseley

A

X-Ray Emission Spectra Experiment

-Caused order number to become atomic number

24
Q

Atomic Number

A

Number of protons

25
Q

Mass number

A

Protons plus neutrons

26
Q

Isotopes

A

Same number of protons, different number of neutrons

27
Q

Nuclide

A

Atom of a specific isotope

28
Q

Percent abundance

A

Use x-1

29
Q

Specific heat

A

Amount of heat needed to raise the temperature of 1 g of the element by 1 degree Celcius

30
Q

Berzelius

A

Published first accurate table of atomic masses

31
Q

Mendeleev

A

First periodic table

32
Q

Columns

A

Groups

33
Q

Periods

A

Rows

34
Q

Metal

A

Left/middle of table

35
Q

Nonmetal

A

Upper right of table

INCLUDES HYDROGEN

36
Q

Group 1

A

Alkali Metals

37
Q

Group 2

A

Alkaline Earth Metals

38
Q

Group 17

A

Halogens (salt formers)

39
Q

Group 18

A

Noble gases

40
Q

Molecular vs. Empirical formula

A

Empirical is simplest numbers possible

Ex. C6H12O6 vs. CH2O

41
Q

Cation

A

Positive Ion (smaller than neutral atom)

42
Q

Anion

A

Negative Ion (larger than neutral atom)

43
Q

Ionic Compound

A

Compounds composed of oppositely charged ions between metal and nonmetal

44
Q

NH3

A

Ammonia

45
Q

PH3

A

Phosphine

46
Q

N2H4

A

Hydrazine

47
Q

Name the cation

A
  • Same name as metal

- If metal can form several cations, use Roman numerals

48
Q

Name the anion

A

Named using “ide” suffix

49
Q

Naming binary molecular compounds (meaning there’s something like (l) or (s) or (aq))

A
  • Name first element
  • Name second with “ide” ending
  • Use prefixes with both names to indicate number of atoms
  • If first atom is hydrogen then no prefixes
50
Q

Prefixes to indicate number of atoms in compound

A 
1 mono
2 di
3 tri
4 tetra
5 penta
6 hexa
7 hepta
8 octa
9 nona
10 deca
51
Q

Naming acids

A
  • Acids whose anion name ends in ide, put hydro in front of anion name and change ide to ic
  • Acids whose anion name ends in ate change ate to ic
  • Acids whose anion name ends in ite change ite to ous
52
Q

Complete combustion

A

Only CO2 and H2O are produced

53
Q

Incomplete combustion

A

Some CO and some C is produced as well as H2O

54
Q

Avogadro’s number

A

6.022 x 10^23

55
Q

Molar Mass

A

Mass of one mole of an element

AP Chemistry (6 decks)

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