Chemistry Quarter 1 Exam Review Flashcards

1
Q

system of measurement primarily used in science

A

metric system

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2
Q

unit of time in metric system

A

seconds

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3
Q

the purpose of scientific notation

A

makes large numbers more manageable

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4
Q

REVIEW SECTION 1.3 for SIG FIG RULES

A
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5
Q

REVIEW METRIC PREFIXES (pg. 7)

A
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6
Q

what is matter?

A

anything that has mass and occupies space

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7
Q

four states of matter

A

solid
liquid
gas
plasma

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8
Q

smallest individual particle

A

atom

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9
Q

smallest individual part of a compound

A

molecule

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10
Q

cannot be broken down further chemically

A

element

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11
Q

KNOW ELEMENTS AND SYMBOLS (pg. 19)

A
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12
Q

homogenous mixture vs. heterogenous mixture

A

homogenous is all uniform in color
heterogenous has phases of color; not uniform

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13
Q

a homogenous mixture is also known as a

A

solution

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14
Q

atomic theory–

A
  1. every element consists of tiny, indivisible, indestructible particles called atoms (FALSE; atoms are destructible)
  2. all of the atoms of a particular element have the same size, mass, and chemical behavior (FALSE; atoms vary slightly in mass)
  3. differences in properties of elements result from differences in the atoms of the elements
  4. the atoms of the elements combined in a compound are combined in a definite ratio
  5. a chemical reaction is the result of rearrangement, combination, or separation of atoms
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15
Q

states that the ratios of the masses of each element in a given compound are always the same

A

law of definite composition

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16
Q

states that when two elements can combine to form more than one compound, the masses of one element that combine with a fixed amount of the other element are in a ratio of small whole numbers

A

law of multiple proportions

17
Q

properties determined by reactions, flammability, acidity

A

chemical properties

18
Q

properties determined by looking; color, state of matter, mass

A

physical properties

19
Q

proposed the hard-sphere model of the atom (1)

A

Dalton

20
Q

proposed the plum-pudding model of the atom (2)

A

Thompson

21
Q

proposed the planetary model of the atom (3)

A

Rutherford

22
Q

when atoms of the same element differ in number of neutrons

A

isotopes

23
Q

the comparison of protons to electrons; the imbalance of protons to electrons

A

ions

24
Q

positively charged ion

A

cation (excess of protons)

25
Q

negatively charged ion

A

anion (excess of electrons)

26
Q

KNOW HOW TO MATHEMATICALLY FIND # OF PROTONS, ELECTRONS, AND NEUTRONS

A
27
Q

the number of protons

A

atomic number (Z)

28
Q

the sum of the number of protons (Z) and neutrons (N)

A

mass number (A)

29
Q

mass number equation

A

A = Z + N

30
Q

neutron equation

A

N = A - Z

31
Q

the # of electrons is determined by the

A

of protons and the -+ symbol of element

32
Q

means to measure elements

A

stoichiometry

33
Q

a molecular compound consists of

A

two nonmetals

34
Q

ionic compounds consist of

A

at least 1 metal and 1 nonmetal

35
Q

KNOW IONIC COMPOUNDS (pg. 40)

A
36
Q

BE ABLE TO CALCULATE MOLAR MASS AND MOLECULAR MASS

A

same procedure for both– add all the atomic masses of elements

37
Q

Avogadro’s number

A

6.022 x 10^23
a mole of anything
the link between the micro and macro

38
Q
A