Chem 1A, Test 1 Review

Front 1

Chemistry

Back 1

the science that seeks to understand the behavior of matter by studying the behavior of atoms and molecules

Front 2

1. Matter

2. 3 states of matter

Back 2

1. anything that hass mass and occupies space.

2. solid, liquid, gas

Front 3

Solids

Back 3

fixed shape, fixed volume, non compress, non flow

Front 4

Liquids

Back 4

indef shape, fixed volume, non compress, yes flow

Front 5

Gases

Back 5

indef shape, indef volume, yes compress, yes flow

Front 6

Classifications of Matter

1. Pure Substance

2. Mixture

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1. made of one type of particle, all samples show same intensive properties.

2. made of multiple types of particles, may show different intensive properties.

Front 7

Classification of Pure Substances

1. Element

2. Compound

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1. substance that cannot be broken down into simpler substances.

2. substance that can be decomposed, chemical combination of elements, all samples of compounds behave the same way.

Front 8

Classifications of Mixtures

1. Heterogeneous

2. Homogeneous

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1. Made of multiple substances whose presence can be seen, portions of samples have different composition and properties.

2. made of multiple substances but appear as one, all portions of a sample have same composition and properties.

Front 9

Changes in Matter

1. Physical Change

2. Chemical change

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1. alter the state or appearance of matter without altering the composition

2. alter the chemical composition of the matter

Front 10

Properties of matter

1. Physical Properties

2. Chemical properties

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1. can be changed without changing the composition

2. are the characteristics that determine how the composition of matter changes as a result of contact with other matter or the influence of energy

Front 11

Examples

1. Physical changes

2. Chemical changes

Back 11

1. boiling, condensing, melting, freezing, subliming, dissolving

2. rusting, burning, processes that release lots of energy

Front 12

1. Energy

2. Work

3. Force

Back 12

1. The capacity to do work.

2. action of a force applied across a distance

3. a push or a pull on an object, electrostatic force is the push or pull on objects that have an electric charge

Front 13

Energy of Matter

1. Kinetic energy

2. Potential energy

Back 13

1. energy of motion. Motion of the atoms, molecules and subatomic particles. Thermal energy is a form of kinetic energy.

2. Energy stored in matter due to the composition of matter and its position of the universe. Chemical potential energy arises from the electrostatic forces between atoms, molecules and subatomic particles.

Front 14

When reading a measurement

Back 14

use the bottom of the miniscus and don't forget to estimate the last digit

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Density =

Back 15

mass/volume

Front 16

0 degrees C =
1. fahrenheit
2. kelvin

Back 16

1. 32

2. 273

Front 17

100 degrees C =
1. fahrenheit
2. kelvin

Back 17

1. 212

2. 373

Front 18

Fahrenheit to Celsius conversion

Back 18

C = (F-32)
-----------
1.8

Front 19

Celsius to Kelvin conversion

Back 19

K = C+273.15

Front 20

Significant Figures

Back 20

1. all non-zero figures are sig.
2. interior zeroes are sig.
3. leading zeroes are not sig.
4. trailing zeroes are only sig. if they are after a decimal point.
5. exact numbers and conversion factors have an infinite number of sig figs.

Front 21

Significant Figures
1. multiplication/division
2. addition/subtraction

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1. use the same as the measurement with the least number of sig figs
2. use the same number of decimal places as the measurement with the fewest number of decimal places

Front 22

1. Precision

2. Accuracy

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1. an indication of how reproducible a measurement is

2. an indication of how close a measurement comes to the actual value of the quantity

Front 23

Dalton's Atomic Theory

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1. each element is composed of tiny, indestructable particles called atoms
2. all atoms of a given element have the same mass and other properties that distinguish them from atoms of other elements
3. atoms combine in simple whole-number ratios to form molecules of compounds
4. in a chemical reaction, atoms of one element cannot change into atoms of another element

Front 24

Structure of the atom

Back 24

1. the atom contains a tiny dense center called the nucleus
2. nucleus has essentially the entire mass of the atom
3. nucleus is positively charged
4. electrons are dispersed in the empty space of the atom surrounding the nucleus

Front 25

Isotopes

Back 25

the same element can have atoms with different masses called isotopes, weights depend on the number of neutrons, identified by their mass numbers: protons + neutrons

Front 26

1. atomic number

2. mass number

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1. number of protons

2. protons + neutrons

Front 27

Number of
1. protons
2. neutrons

52
Cr
24

Back 27

1. 24

2. 28

Front 28

1. cation

2. anion

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1. when atoms lose electrons they become positively charged ions

2. when atoms gain electrons they become negatively charged ions

Front 29

anions are named by:

F-

Back 29

changing the end of the name to -ide

Flouride

Front 30

cations are named by:

Na+

Back 30

same as the metal they are composed of

sodium ion

Front 31

Periodic table is broken up into:

Back 31

metals, non-metals, metalloids, main group, transition metals.

Front 32

Avogadro"s number

Back 32

6.0221421 x 10^23

Front 33

Ionic charge and the periodic table:
1. metals
2. non-metals

Back 33

1. always positively charged, main group metals charge = group number
2. always negatively charged, charge = group number -8

Front 34

molar mass

Back 34

mass of one mole of atoms or molecules of a particular element or compound

Front 35

Chemical Bonds
1. ionic bonds
2. covalent bonds

Back 35

1. electrons have been transferred between atoms
2. atoms share some of their electrons

Front 36

Chemical Formula
1. Empirical Formula
2. Molecular Formula

Back 36

1. describe the kinds of elements found in the compound and the ratio of their atoms
2. describe the kinds of elements found in the compound and the number of their atoms

Front 37

Atomic elements

Back 37

elements whose particles are single atoms

Front 38

molecular elements

Back 38

elements whose particles are multi-atom molecules

Front 39

molecular compounds

Back 39

compounds whose particles are molecules made of only non-metals

Front 40

ionic compounds

Back 40

metals + non-metals, compounds whose particles are cations and anions

Front 41

writing formulas for ionic compounds

Back 41

1. write the symbol for the metal cation and its charge
2. write symbol for non-metal anion and its charge
3. charge becomes subscript for other ion
4. reduce subscripts to smallest whole number ratio
5. check that the sum of the charges of the cation cancels the sum of the anions

Front 42

Ionic Bonds: Metal and Non-metal

Type I: Metal forms 1 type of Ion only

Back 42

Name of cation +-ide

Ex: CaI2, calcium iodide

Front 43

Ionic Bonds: Metal and Non-metal

Type II: Metal forms more than 1 type of ion

Back 43

Name of cation, charge of cation in roman numerals, + -ide

Ex: FeCl3, iron (III) chloride

Front 44

Covalent Bonds: Molecular bonds between non-metals only

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prefix+name of first element, then prefix+name of second element+-ide

Ex: P2O5, diphosphorus pentoxide

Front 45

Acids: H and one or more non-metals

Binary: Two-element

Back 45

Hydro+base name non-metal + -ic acid

Ex: HCl, hydrochloric acid

Front 46

Acids: H and one or more non-metals

Oxyacids: Contain oxygen and ends in -ate

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Base name of oxyanion + -ic

Ex: H3PO4, phosphoric acid

Front 47

Acids: H and one or more non-metals

Oxyacids: Contain oxygen and ends in -ite

Back 47

Base name of oxyanion + -ous

Ex: H2SO3, sulfurous acid

Front 48

HClO4

Back 48

Perchloric Acid

Front 49

HI

Back 49

Hydroiodic Acid

Front 50

Ca SO4

Back 50

Calcium Sulfate

Front 51

KH2PO4

Back 51

Potassium Dihydrogen Phosphate

Front 52

Sr(OH)2

Back 52

Strontium Hydroxide

Front 53

FeCl3

Back 53

Iron (III) Chloride

Front 54

Cu2SO4

Back 54

Copper (I) Sulfate

Front 55

Co(NO3)2

Back 55

Cobalt (II) Nitrate

Front 56

MnO

Back 56

Magnese (II) Oxide

Front 57

HCl

Back 57

Hydrochloric Acid

Front 58

HNO3

Back 58

Nitric Acid

Front 59

H2SO4

Back 59

Sulfuric Acid

Front 60

HBr

Back 60

Hydrobromic Acid

Front 61

Polyatomic Ions

C2H3O2

Back 61

acetate

Front 62

Polyatomic Ions

CO3

Back 62

carbonate

Front 63

Polyatomic Ions

HCO3

Back 63

hydrogen carbonate

Front 64

Polyatomic Ions

OH

Back 64

hydroxide

Front 65

Polyatomic Ions

NO3

Back 65

nitrate

Front 66

Polyatomic Ions

NO2

Back 66

nitrite

Front 67

Polyatomic Ions

CrO4

Back 67

chromate

Front 68

Polyatomic Ions

Cr2O7

Back 68

dichromate

Front 69

Polyatomic Ions

NH4

Back 69

ammonium

Front 70

Polyatomic Ions

ClO

Back 70

hypochlorite

Front 71

Polyatomic Ions

ClO2

Back 71

chlorite

Front 72

Polyatomic Ions

ClO3

Back 72

chlorate

Front 73

Polyatomic Ions

ClO4

Back 73

perchlorate

Front 74

Polyatomic Ions

SO4

Back 74

sulfate

Front 75

Polyatomic Ions

SO3

Back 75

sulfite

Front 76

Polyatomic Ions

HSO4

Back 76

hydrogen sulfate

Front 77

Polyatomic Ions

HSO3

Back 77

hydrogen sulfite

Front 78

1. hydrate

2. anhydrate

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1. ionic compounds containing a specific number of H2O molecules for each formula unit, 6H2O = hexahydrate, 1/2 H2O = hemihydrate
2. ionic compounds not containing a number of H2O molecules per formula unit

Front 79

writing names of molecular compounds of 2 non-metals

Back 79

1. write name of first element
2. name of second element + -ide suffix
3. use a prefix in front of each name to indicate the number of atoms

Front 80

Formula Mass

Back 80

Mass of one individual molecule or formula unit.

H2O = 2(1.008)+16.00 = 18.02amu

Front 81

Molar Mass

Back 81

identical to formula mass just in units of g/mole

Front 82

Percent Composition:

CaCl2 percent of Ca?

Back 82

molar mass Ca
---------------------------- x 100
molar mass CaCl2

Front 83

Given 2.4g Na, NaCl is 39% Na. Find mass of NaCl containing 2.4g of Na

Back 83

1. 100g NaCl contains 39g Na and 61g Cl so...

100g NaCl
2. 2.4g Na x ------------------ =
39g Na

Front 84

Finding Empirical Formula

Back 84

1. convert percentages to grams
2. convert grams to moles
3. write a pseudoformula using moles as subscripts
4. divide by smallest number of moles
5. multiply all mole ratios by number to make all whole numbers.