Chemistry Chapter 1,2

Front 1

Matter

Back 1

anything that has mass and takes up space

Front 2

Weight

Back 2

pull of gravity on stuff

Front 3

Mass

Back 3

amount of stuff

Front 4

Scientific Method (Steps)

Back 4

a systemic approach to research
- identify the problem
- make a hypothesis
- perform the experiment: making observations, recording data
- make a conclusion

Front 5

chemistry

Back 5

study of matter and the changes it undergoes

Front 6

substance

Back 6

matter with definite composition and has distinct properties (H2O or Au)

Front 7

mixture

Back 7

2 or more substances (NaCl)

Front 8

Homogeneous mixture

Back 8

uniform, you can't tell the difference

Front 9

Heterogenous mixture

Back 9

you can tell the difference between the substances

Front 10

Element

Back 10

substance that cannot be separated into a simpler substance by chemical means

Front 11

Compound

Back 11

2 or more elements "bonded" together
can be separated by chemical means and is found in fixed proportions

Front 12

physical property

Back 12

observed without changing the composition (boiling water)

Front 13

chemical property

Back 13

perform a chemical reaction

Front 14

extensive property

Back 14

depends on the amount (mass, volume, length)

Front 15

intensive property

Back 15

independent of the amount (density, color, boiling point/melting point)

Front 16

macroscopic properties

Back 16

observed directly

Front 17

microscopic properties

Back 17

cannot be directly observed (on the atomic or molecular scale)

Front 18

Significant Figures: digit rules

Back 18

1. all numbers that aren't zero count
2. trailing zeros after decimal points count (1.0)
3. place holder zeroes don't count (100 has only one sigfig)
4. captive zeros count (a zero between 2 sigfigs like 1.01)

Front 19

Significant Figures: mult/division

Back 19

use the lowest number of SIGFIGS

Front 20

Significant Figures: add/sub

Back 20

use the lowest number of DECIMALS

Front 21

accuracy

Back 21

tells us how close a measurement is to the TRUE VALUE of the quantity that was measured

Front 22

precision

Back 22

refers to how CLOSELY two or more measurement of the same quantity agree with one another

Front 23

percent error

Back 23

how good/bad results are
= abs(your value-actual value)/ actual x 100%

Front 24

Democritus

Back 24

matter is composed of smaller particles called atomos

Front 25

Dalton's Atomic Theory

Back 25

1. elements are composed of atoms
2. different elements are different atoms
3. compounds are formed when different elements come together and have fixed ratios
4. chemical reaction is a rearrangement of atoms

Front 26

isotope

Back 26

same element, different atomic mass
same number of protons, different number of neutrons

Front 27

Law of definite proportions

Back 27

compounds always contain the same elements in definite proportions by mass

Front 28

Law of multiple proportions

Back 28

in a series of compounds with the same elements, the second element always combines with 1 gram of the 1st element in a whole number ratio. (H2O2 is H2O)

Front 29

Law of conservation of matter(energy)

Back 29

you cannot create or destroy matter/energy

Front 30

protons (mass, charge, location?)

Back 30

mass: 1 amu
charge: +1
location: nucleus

Front 31

neutrons (mass, charge, location?)

Back 31

1 amu.
neutral
nucleus

Front 32

electrons (mass, charge, location?)

Back 32

0 mass
-1
outside the nucleus

Front 33

JJ Thompson

Back 33

He determine a charge to mass ratio = -1.76 x 10^8 coulombs/gram
- using a cathode ray tube (glass tube with mercury vapor) and 2 electrically charged plates and magnet on the outside
- Cathode ray attracts positive charges and repels negative
-electrons flowed toward negative

Front 34

Robert Millikan

Back 34

determined the exact charge of an electron with his oil drop experiment
- mass of an electron= 9.11 x 10^-31

Front 35

Becquerel and Radioactivity

Back 35

- put a rock on photographic plate, saw it was exposed to light from the rock

Radioactivity: spontaneous emission of particles and/or radiation

Front 36

Types of Radioactivity (Alpha)

Back 36

Charge: +2
Mass: 4 amu
Particles: 4/2 He nucleus

least penetration power (stops at paper)

Front 37

Types of Radioactivity (Beta)

Back 37

charge -1
mass 0 amu
particles: electron

middle penetration power (stops at aluminum foil)

Front 38

Types of Radioactivity (Gamma)

Back 38

0 charge
0 mass
pure energy particles

most penetration power (stops at lead or concrete)

Front 39

Rutherford and his 3 observations/conclusions

Back 39

made observations of alpha scattering using gold foil and a glowing detector for alpha particles that reach the end

1. most alphas went straight through --> atoms are made of mostly empty space.
2. some alphas were deflected --> nucleus was positively charged.
3. few alphas were bounced straight back--> nucleus was very small and very dense.

Front 40

Chadwick

Back 40

his experiments showed that NEUTRONS have a mass slightly greater than protons

Front 41

atomic number

Back 41

number of protons/electrons in the nucleus

Front 42

mass number

Back 42

total number of neutrons and protons present in the nucleus

Front 43

mass number - atomic number =

Back 43

neutrons

Front 44

Mass spectrophometer

Back 44

measures mass of isotopes
(looks like a slide)
- smaller masses will get deflected the most
- larger masses will get less deflected

Front 45

Average Atomic Mass

Back 45

weighted average of all known isotopes and abundances

Front 46

groups (periodic table)

Back 46

columns!

Front 47

periods (periodic table)

Back 47

rows!

Front 48

Group 1

Back 48

Alkali metals; most reactive

Front 49

Group 2

Back 49

Alkaline earth metals

Front 50

Groups 3-12

Back 50

Transition metals: are most likely to form cations with different charges

Front 51

Group 16

Back 51

Calcogen (chalk forming)

Front 52

Group 17

Back 52

Halogens: most reactive NONMETALS

Front 53

Group 18

Back 53

Noble Gases

Front 54

Ion

Back 54

charged atom

Front 55

Cation

Back 55

positive ion (less electrons than protons)

K+ has 19 protons, but 18 electrons

Front 56

Anion

Back 56

negative ion (too many electrons)

Cl- has 17 protons, but 18 electrons

Front 57

Metals are

Back 57

LOSERS
will lose electrons

Front 58

Nonmetals are

Back 58

GAINERS

Front 59

Ionic compounds

Back 59

are formed when ions stick together
metal -- nonmetal

Front 60

Molecular compounds

Back 60

nonmetals -- nonmetals

Front 61

Metalloids

Back 61

Elements that have properties of both metals and nonmetals

the steps on the period table

Front 62

Molecule vs. Compound

Back 62

Molecules are 2 or more ATOMS bonded together like H2

Compounds are 2 or more ELEMENTS bonded together like H2O

Front 63

Only 2 liquids at room temperature?

Back 63

Bromine, mercury

Front 64

Molecular Formula

Back 64

tell you the number and type of atoms present (H2O)

Front 65

Empirical Formula

Back 65

simplest whole number ratio of the atoms, THE MOST REDUCED

instead of C6H12O6--> CH2O

Front 66

Structural Formula

Back 66

arrangement of atoms in space

Front 67

Stock system

Back 67

when there is a choice of oxidation numbers for the 1st atom, must denote the oxidation number with Roman numerals

Front 68

Acids

Back 68

produce H+ ions (usually Hydrogen in the front)

Front 69

Binary Acids

Back 69

H_____
hydro___ic acid

Front 70

Terniary acids

Back 70

H____O
(usually looking at the poly table)

ate --> ic acid
ite--> ous acid

Front 71

Bases

Back 71

produce OH- ions
- might have to use stock system

usually ends in hydroxide

Front 72

Allotrope

Back 72

more than one natural form of an element
(ex. Carbon = bucky ball, diamond, graphite)
(Oxygen = o2, o3)

Front 73

Hydrates

How do you name hydrates?

Back 73

water trapped within a crystal
BaCl2 (dot) 4H2O

for every bacl2, there are 4 h2os trapped within a crystal.

Barium chloride tetra hydrate

Front 74

1,2,3,4,5,6,7,8,9,10

Back 74

mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca