Chem 110

Front 1

What is the difference b/t pure substances and Mixtures

Back 1

A mixture can be made up of 2 or more substances and do not have exact properties as their compositions can vary. Pure substances have fixed ratios. Mix can change it's state over a range of temps but pure substances will only change at fixed boiling points and melting points.

Front 2

What is the difference b/t elements and compounds?

Back 2

Elements can't be separated whereas compounds can be.

Front 3

What is the difference between homogenous and heterogenous mixtures?

Back 3

Homo. mixtures are uniformed through out. Ex: salt Heterogeneous is non composition such as soil and water.

Front 4

List the states of Solids, Liquids, and Gases

Back 4

Liquids have definite volume and but not shape. Gas have no shape nor volume. Solids have definite shape and volume

Front 5

What is the difference b/t chem and physical changes in a reaction.

Back 5

Chem reaction when the outcome has different compounds than when it start. Ex: Porpane Physical reaction the composition stays the same but the physical properties change. EX: Rubbing alcohol on the skin.

Front 6

Why is the decimal system important?

Back 6

The decimal point shows the relationship b/t measurements

Front 7

What is the relationship b/w liter and cm3 and ml and cm3

Back 7

1000ml=1 Liter
1cm3 = 1ml

Front 8

How is Volume typically measured?

Back 8

mL

Front 9

What is the difference b/t exact numbers and non-exact numbers

Back 9

Exact numbers have no uncertainty 12 ft= 1 foot. Inexact numbers have a degree of uncertainty. Ex: All measurements

Front 10

1 mile = ___ Km

Back 10

1.609 Km

Front 11

1 lb= ___ g

Back 11

453.6 g

Front 12

1 kg = _____ lbs

Back 12

2.205 lbs

Front 13

1 0z =_____ g

Back 13

28.35g

Front 14

1 meter = _____ inches

Back 14

39.37

Front 15

1 gallon = _____ Liters

Back 15

3.785

Front 16

1 in =_________ cm

Back 16

2.54cm

Front 17

1 calorie = ________j

Back 17

4.148J

Front 18

Heat, electricity, and light are considered mass. T/F

Back 18

False

Front 19

How is gas typically measured?

Back 19

mL or L

Front 20

How is K calculated?

Back 20

C + 273

Front 21

What is the formula to calculate C into F

Back 21

C= 5/9 (F - 32)

Front 22

calculate F-C

Back 22

F= 9/5(C) + 32

Front 23

Formula for Density

Back 23

D= M/V

Front 24

Formula for Volume

Back 24

V= M/D

Front 25

Formula for Mass

Back 25

M= D*V

Front 26

Define Density.

Back 26

Is defined as its mass per volume unit.

Front 27

Specific Gravity is the same as what?

Back 27

Density

Front 28

What is boiling point for F?

Back 28

212F

Front 29

What is the freezing point in F?

Back 29

32F

Front 30

What is the boiling point of C

Back 30

100

Front 31

What is the Freezing Point in C?

Back 31

0

Front 32

What is the boiling point in K

Back 32

100 + 273= 373

Front 33

What is the freezing in K?

Back 33

273

Front 34

Normal body temp in K

Back 34

310

Front 35

What is the highest degree in K

Back 35

373

Front 36

What is the lowest temperature in K?

Back 36

0

Front 37

1 Calorie =________J

Back 37

4.148 J

Front 38

What is the formula for Specific Heat

Back 38

SH= m x g x ch in Temp

Front 39

Formula for Change in Temp

Back 39

CT = Amount of heat/ M x g

Front 40

Formula for Amount of Heat

Back 40

Amount of Heat = SH x M x Ch in Temp

Front 41

Is Bronze is mixture, compound or element?

Back 41

Mixture:

Front 42

Ag

Back 42

Silver

Front 43

Al

Back 43

Aluminum

Front 44

Ar

Back 44

Argon

Front 45

Au

Back 45

Gold

Front 46

Boron

Back 46

B

Front 47

Gold

Back 47

Au

Front 48

Cu

Back 48

Copper

Front 49

Ca

Back 49

Calcium

Front 50

Cl

Back 50

Clorine

Front 51

Ba

Back 51

Barium

Front 52

Be

Back 52

Beryllium

Front 53

Br

Back 53

Bromine

Front 54

platinum

Back 54

Pl

Front 55

Mercury

Back 55

Hg

Front 56

What does the chemical formula tell you?

Back 56

Gives you the elements involved and their ratio to each other.

Front 57

Explain Daltons Theory

Back 57

Matter is composed of atoms. In a chemical reaction atoms are combined, separated, or rearranged but NEVER changed into atoms of another element.

Front 58

What is the law of conservation?

Back 58

Matter can't be destroyed. A chemical reaction only changes the attachments of the atom and doesn't destroy the atom.

Front 59

What is the complete chemical symbol notation.

Back 59

As it appears on the P. Table

Front 60

What are the physical properties of alkaline metals

Back 60

Shinny, malleable, soft, colored when they burn

Front 61

List the properties of Halogens

Back 61

Are colored and are used for disinfectants.

Front 62

How does the first row of elements compare to the last row of elements.

Back 62

The first row of elements are extremely active whereas the noble gases are not.

Front 63

What is an alloy metal

Back 63

Metals that melt / dissolve into one another. Brass and Zn = Bronze

Front 64

List the recurring properties of Halogens

Back 64

They are colored and react to Na and have low melting points and boiling points.

Front 65

List the differences b/w metals, metalloids, and nonmetals

Back 65

metals=shinny, electrical conductor, malleable high melting points. Non metals are dull brittle and poor electrical conductors, may be liq solids or gases at room temp. Metalloids have characteristics of both

Front 66

Which metalloid is a semiconductor of electricity

Back 66

Silicon

Front 67

What factor dictates Boiling and melting points of Halogens and Noble gases?

Back 67

Going down the P. Table getting bigger which takes longer.

Front 68

What is the factor that dictates mp and bp of alkaline metals

Back 68

As you go up the Table the boiling points increase because the attraction of the P and e.

Front 69

What factor dictates the amount of ionization needed to remove an e from an atom

Back 69

The further the e are away from the nucleus the less energy it takes to remove the e. And the further you move to the right to more difficult due to the added protons.

Front 70

1 km = __ m

Back 70

1000m

Front 71

1mL =____L

Back 71

0.001L

Front 72

1 Kg= ___lbs

Back 72

2.205 lbs

Front 73

1 gallon = ___ L

Back 73

3.785

Front 74

1 lb=___ g

Back 74

453.6 g

Front 75

1 m = ___in

Back 75

39.37 inches

Front 76

NH4+

Back 76

Ammonium

Front 77

OH-

Back 77

Hydroxide

Front 78

NO2-

Back 78

Nitrite

Front 79

NO3-

Back 79

Nitrate

Front 80

CH3OO-

Back 80

acetate

Front 81

CN-

Back 81

Cyanide

Front 82

MnO4-

Back 82

Permanganate

Front 83

CrO4 2-

Back 83

Chromate

Front 84

CrO72-

Back 84

Dichromate

Front 85

HCO3-

Back 85

Hydrogen Carbonate

Front 86

SO3 2-

Back 86

Sulfite

Front 87

HSO3-

Back 87

Hydrogen sulfite

Front 88

SO4 2-

Back 88

Sulfate

Front 89

HSO 4-

Back 89

Hydrogen Sulfate

Front 90

PO4 3-

Back 90

Phosphate