Ch1-2

Question 1

experiment

Answer 1

observation of natural phenomena carried out in a controlled manner

Question 2

law

Answer 2

observations in nature that are repeated and give the same result

Question 3

mass

Answer 3

the quantity of matter in a material

Question 4

weight

Answer 4

the force of gravity exerted on an object

Question 5

matter

Answer 5

whatever occupies space and can be perceived by our senses

Question 6

law of conservation of mass

Answer 6

Lavoisier stated that total mass remains constant during a chemical reaction

Question 7

fixed shape/fixed volume/neither

1) solid
2) liquid
3) gas

Answer 7

1) fixed shape, fixed volume
2) no fixed shape, fixed volume
3) no fixed shape, no fixed volume

Question 8

1) physical change
vs
2) chemical change

Answer 8

1) change in the form of matter but not in its chemical identity
2) change in which one or more kinds of matter are transformed into a new kind of matter

Question 9

distillation

Answer 9

process of separating an easily vaporized liquid from another substance (water from sodium chloride)

Question 10

1) physical property
vs
2) chemical property

Answer 10

1) characteristic that can be observed without changing chemical identity
(color)
2) a characteristic involving its chemical change
(chemical property of iron = rust)

Question 11

mixtures are separated by a ____ property

Answer 11

physical

Question 12

elements in a compound are separated by a ____ property

Answer 12

chemical

Question 13

1) substance
vs
2) element

Answer 13

1) kind of matter that cannot be separated into other matter by physical processes (EX: sodium chloride only separated by chemical)
2) a substance that cannot be decomposed by any chemical processes into simpler substances
(EX: arsenic, mercury, etc)

Question 14

1) compound
vs
2) mixture

Answer 14

1) a substance composed of two or more elements chemically combined; can be separated
(water = hydrogen + oxygen)

2) the combination of two or more substances in which substances retain their distinct properties
(dissolving salt in water, can be distilled)

Question 15

1) law of definite proportions
vs
2) law of multiple proportions

Answer 15

1) a pure compound always contains constant proportions of the elements by mass
2) when two elements form more than one compound, the masses of one element have a fixed ratio for the mass of the other element
(ex: CO 2:1 mass, CO2 2:1 mass)

Question 16

a solution is also known as

Answer 16

a homogeneous mixture

Question 17

602200 in scientific notation

Answer 17

6.022 x 10^5

Question 18

.000166 in scientific notation

Answer 18

1.66 x 10^-4

Question 19

precision vs accuracy

Answer 19

precision = closeness of a set of values to one another

accuracy = closeness of a single measurement to correct value

Question 20

350 + 93,000,000 in sig figs

Answer 20

93,000,000 because since 100,000 is next biggest column and 350 doesn’t fit there, it is not added on

Question 21

measured number vs exact number

Answer 21

1) measured = number which is observed and recorded in an experiment
2) recorded= number that arises when you count items (9 coins)

Question 22

prefixes

Answer 22

kilo (10^3)
hecto (10^2)
deca (10^1)
UNIT
deci (10^-1)
centi (10^-2)
milli (10^-3)
micro (10^-6)
nano (10^-9)

Question 23

1 mL =

Answer 23

1 m^3

Question 24

atomic theory

Answer 24

an explanation of the structure of matter

Question 25

4 main points of dalton’s atomic theory

Answer 25

1) elements are composed of extremely small particles called atoms 2) atoms of a given element are identical, having the same size, mass, and chemical properties 3) compounds are composed of atoms of more than one element (equal ratio) 4) a reaction only involves the separation, combination or rearrangement of atoms

Question 26

atom-

Answer 26

an extremely small particle of matter

Question 27

chemical reaction-

Answer 27

the rearrangement of atoms present in the reactants

Question 28

nucleus-

Answer 28

the atom’s central core, positively charged

Question 29

what did each person discover? 1) chadwick 2) rutherford 3) thomson 4) dalton

Answer 29

1) neutrons 2) nucleus 3) electrons 4) atom

Question 30

atomic number

Answer 30

number of protons

Question 31

mass number

Answer 31

total number of protons and neutrons

Question 32

isotopes

Answer 32

atoms whose nuclei have same atomic number but different mass numbers (neutron numbers)

Question 33

how does dalton use the laws of chemical composition in his atomic theory?

Answer 33

1) elements are composed of the same atom = law of definite proportions 2) a reaction only involves the separation, combination or rearrangement of atoms = law of conservation of mass

Question 34

what points in john dalton’s atomic theory are still considered valid as he presented them?

Answer 34

atoms are the smallest particles

Question 35

describe ONE discovery that changed the view of the atom and how it changed the atomic view

Answer 35

not all elements are identical = isotopes

Question 36

fractional abundance

Answer 36

the fraction of the total number of atoms that is composed of an isotope

Question 37

an atom that is most abundant is ____

Answer 37

the closest to its average atomic mass

Question 38

period vs group

Answer 38

period = horizontal group = vertical

Question 39

metal vs nonmetal vs metalloid

Answer 39

1) metal = solids at room temp 2) nonmetal = gases/solids at room temp 3) metalloid = has both metallic and nonmetallic properties

Question 40

1) molecular formula vs 2) structural formula

Answer 40

1) gives the exact number of different atoms of an element in a molecule (H2O) 2) shows how the atoms are bonded together in a molecule (H-O-H)

Question 41

molecule-

Answer 41

definite group of atoms chemically bonded together by attractive forces

Question 42

polymers vs monomers

Answer 42

large polymers are made of smaller monomers

Question 43

ion

Answer 43

an electrically charged particle obtained from an atom or chemically bonded group of atoms by adding or removing atoms

Question 44

anion vs cation

Answer 44

1) anion- negatively charged ion, when an atom gains an electron 2) cation- positively charged ion, when an atom loses an electron

Question 45

monatomic ion vs polyatomic ion

Answer 45

1) single atom ion (H+) | 2) ions made up of more than one atom (NO2-)

Question 46

ionic compounds vs molecular compounds

Answer 46

1) between two metals (transfer electrons) | 2) between two or more nonmetals (share electrons)

Question 47

differentiate between an isotope’s atomic mass and an element’s average atomic mass (atomic weight)

Answer 47

1) atomic mass is total number of protons and neutrons | 2) average atomic mass is the sum of all of the isotopes masses and their fractional abundance’s

Question 48

organic compounds

Answer 48

molecular substances that contain carbon combined with other elements (H, O, N)

Question 49

hydrocarbons

Answer 49

compounds containing only hydrogen carbon (CH4 methane)

Question 50

functional group

Answer 50

a reactive portion of a molecule that undergoes predictable reactions

Question 51

chemical nomenclature

Answer 51

the systemic naming of chemical compounds

Question 52

inorganic compounds

Answer 52

compounds composed of elements other than carbon

Question 53

chemical equation

Answer 53

the symbolic representation of a chemical reaction in terms of chemical formulas

Question 54

pure water is an example of a

Answer 54

compound

Question 55

since the sample of salt and water tastes the same from the top and bottom of the container it is an example of a

Answer 55

homogenous mixture

Question 56

it is cold when it is 32 degrees outside

Answer 56

false

Question 57

a measurement is a number

Answer 57

false

Question 58

the formula of the ionic compound formed by (Na, Group IA) and oxygen (O, Group VIA) is

Answer 58

Na2O