Chemistry Test 1

Front 1

Steps of the Scientific Method

Back 1

1

Front 2

Difference between observations and conclusions

Back 2

1

Front 3

Describe element

Back 3

a single type of atom

Front 4

Describe compounds

Back 4

a pure substance that contains more than one element

Front 5

Homogenous mixture

Back 5

uniform mixtures where the composition is the same throughout

Front 6

Heterogeneous mixture

Back 6

mixture where the composition varies throughout

Front 7

273 degrees kelvin =

Back 7

0 degrees celsius

Front 8

How many sig figs
1. .0023000
2. 1004
3. 1000.00

Back 8

1. 5
2. 4
3. 6

Front 9

when adding or subtracting sig figs

Back 9

you must have the same # of decimal places as the smaller one

Front 10

when multiplying/dividing sig figs

Back 10

must have the same # of sig figs as the smaller sig fig number

Front 11

Density equation

Back 11

D=M/V

Front 12

Group 1A name

Back 12

Alkali metals

Front 13

Group 2A name

Back 13

Alkaline earth metals

Front 14

Group 7A name

Back 14

Halogens

Front 15

Group 8A name

Back 15

Noble gases

Front 16

Dalton's theory of atoms

Back 16

1. An element is composed of atoms. Different elements have different properties because they have different atoms
2. Chemical reactions rearrange combinations of atoms. Atoms dont disappear or change into other kinds of atoms when a reaction occurs
3. Compounds are composed of two or more elements
4. A sample of a given compound will have a composition that will be identical to another sample of that same compound. The ratios of atoms will be whole numbers.

Front 17

Define Nucleus

Back 17

Center of atom

Contains protons and neutrons

Front 18

Proton

Back 18

positively charged particle

Front 19

neutron

Back 19

neutrally charged particle

Front 20

electron

Back 20

negatively charged particle

Front 21

Atomic notation

Back 21

1

Front 22

Define cation

Back 22

positively charged ion

Front 23

Define anion

Back 23

negatively charged ion

usually nonmetals

Front 24

Define molecular compound

Back 24

formed by the sharing of similary charged ions

Front 25

Define ionic compound

Back 25

held together by forces between oppositely charged ions.

Front 26

Define Isotope

Back 26

An atom that has a different # of neutrons that another atom with the same # of atoms

Front 27

Alpha radiation

Back 27

when an element shoots two protons and neutrons out of its nucleus, forming a new element and a helium particle

Front 28

Alpha radiation symbol

Back 28

fish facing left

Front 29

Beta radiation

Back 29

where there are too many neutrons, so an electron contained within the neutron is ejected from it, causing it to become a proton

Front 30

Beta radiation symbol

Back 30

B with tail

Front 31

gamma radiaton

Back 31

pure energy

Front 32

gamma radiation symbol

Back 32

fish facing down

Front 33

Binary molecular compounds

Back 33

when two nonmetals combine with each other.

Must put number prefixs on both, second element ends in -ide

Front 34

acetate

Back 34

C2H3O2

- charge

Front 35

nitrate

Back 35

NO3

- charge

Front 36

nitrite

Back 36

NO2

- charge

Front 37

carbonate

Back 37

CO3

2- charge

Front 38

sulfite

Back 38

SO3

2- charge

Front 39

phosphate

Back 39

PO4

3- charge

Front 40

hydroxide

Back 40

OH

- charge

Front 41

cyanide

Back 41

CN

- charge

Front 42

sulfate

Back 42

SO4

2- charge

Front 43

permanganate

Back 43

MnO4

- charge

Front 44

Ions with hydrogen attached

Back 44

hydrogen is put before the anion

Front 45

ClO4

Back 45

perchlorate

- charge

Front 46

ClO3

Back 46

chlorate

- charge

Front 47

ClO2

Back 47

chlorite

- charge

Front 48

ClO

Back 48

hypochlorite

- charge

Front 49

Naming ionic compounds with transition elements

Back 49

need to include charge

Front 50

Acids

-ides become
- ates become
-ites become

Back 50

hydro -ic
-ic
-ous