Chapter 1+2+3

Question 1

Law

Answer 1

Summarizes what happens

Question 2

Theory/model

Answer 2

Provides an explanation

Question 3

Filtration

Answer 3

Separates insoluble solid from liquid or solution

Question 4

Distillation

Answer 4

Uses different boiling points to separate mixtures

Question 5

Crystallization

Answer 5

Separates using differences in solubility

Question 6

Chromatography

Answer 6

Separates using differences in polarity

Question 7

Extraction

Answer 7

• Separates using differences in polarity

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

Question 8

Kelvin

Answer 8

K = C + 273

Question 9

Fahrenheit

Answer 9

F = 1.8C +32

Question 10

Centimeter

Answer 10

M x 10^-2

Question 11

Millimeter

Answer 11

M x 10^-3

Question 12

Micrometer

Answer 12

M x 10^-6

Question 13

Nanometer

Answer 13

M x 10^-9

Question 14

Dalton’s Early Atomic Theory

Answer 14

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

Question 15

Law of Conservation of Mass

Answer 15

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

Question 16

Law of Constant Composition

Answer 16

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

Question 17

Law of Multiple Proportions

Answer 17

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

Question 18

J.J. Thomson

Answer 18

Cathode Ray Tube Experiments

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

Question 19

R. Millikan

Answer 19

Oil Drop Experiment

-Found charge of an electron

Question 20

Henri Becquerel

Answer 20

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

Question 21

E. Rutherford

Answer 21

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

Question 22

J. Balmer

Answer 22

Visible Light Emission Spectra Experiments

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

Question 23

H. Moseley

Answer 23

X-Ray Emission Spectra Experiment

-Caused order number to become atomic number

Question 24

Atomic Number

Answer 24

Number of protons

Question 25

Mass number

Answer 25

Protons plus neutrons

Question 26

Isotopes

Answer 26

Same number of protons, different number of neutrons

Question 27

Nuclide

Answer 27

Atom of a specific isotope

Question 28

Percent abundance

Answer 28

Use x-1

Question 29

Specific heat

Answer 29

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

Question 30

Berzelius

Answer 30

Published first accurate table of atomic masses

Question 31

Mendeleev

Answer 31

First periodic table

Question 32

Columns

Answer 32

Groups

Question 33

Periods

Answer 33

Rows

Question 34

Metal

Answer 34

Left/middle of table

Question 35

Nonmetal

Answer 35

Upper right of table | INCLUDES HYDROGEN

Question 36

Group 1

Answer 36

Alkali Metals

Question 37

Group 2

Answer 37

Alkaline Earth Metals

Question 38

Group 17

Answer 38

Halogens (salt formers)

Question 39

Group 18

Answer 39

Noble gases

Question 40

Molecular vs. Empirical formula

Answer 40

Empirical is simplest numbers possible | Ex. C6H12O6 vs. CH2O

Question 41

Cation

Answer 41

Positive Ion (smaller than neutral atom)

Question 42

Anion

Answer 42

Negative Ion (larger than neutral atom)

Question 43

Ionic Compound

Answer 43

Compounds composed of oppositely charged ions between metal and nonmetal

Question 44

NH3

Answer 44

Ammonia

Question 45

PH3

Answer 45

Phosphine

Question 46

N2H4

Answer 46

Hydrazine

Question 47

Name the cation

Answer 47

- Same name as metal | - If metal can form several cations, use Roman numerals

Question 48

Name the anion

Answer 48

Named using "ide" suffix

Question 49

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

Answer 49

- 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

Question 50

Prefixes to indicate number of atoms in compound

Answer 50

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

Question 51

Naming acids

Answer 51

- 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

Question 52

Complete combustion

Answer 52

Only CO2 and H2O are produced

Question 53

Incomplete combustion

Answer 53

Some CO and some C is produced as well as H2O

Question 54

Avogadro's number

Answer 54

6.022 x 10^23

Question 55

Molar Mass

Answer 55

Mass of one mole of an element