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CHEM 120 > UNIT 1 > Flashcards

UNIT 1 Flashcards

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1
Q

define chemistry

A

the study of interactions of matter with other matter & with energy

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2
Q

define matter

A

anything that has mass and takes up space

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3
Q

define physical properties

A

characteristics of matter that describe matter as it exists, phase (or state) of matter
ex: density, color, melting

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4
Q

define physical change

A

occurs when a sample of matter changes one or more of its physical properties, does NOT affect the chemical composition of matter
- formation of a mixture

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5
Q

define chemical change

A

formation of a compound

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6
Q

define element

A

simplest type of chemical substance, cannot be broken down into simpler chemical substances by ordinary chemical means

ex: iron nail

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7
Q

compound

A

a combination of 1 or more element

ex: water (H20)

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8
Q

mixtures

A

physical combination of more than 1 substance that aren’t chemically joined
ex: salt water

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9
Q

define heterogeneous mixture

A

composed of 2 or more substances, not evenly distributed

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10
Q

define homogenous/solution

A

combination of 2 or more substances evenly mixed

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11
Q

define metal

A

element that conducts electricity and heat well; to the left of the metalloid line

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12
Q

characteristics of a metal

A
  • solid at room temp
  • shiny/lustrous
  • ductile: can be drawn into wires
  • malleable: can be beaten in thin sheet
  • conduct heat and electricity
  • high densities & melting point
  • lose electrons & form positive ions
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13
Q

define nonmental

A

an element that is brittle when solid, does NOT conduct electricity or heat very well; to the right of metalloid line

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14
Q

characteristics of a nonmetal

A
  • low melting & boiling point
  • brittle, dull
  • insulating (cannot conduct electricity)
  • gain electrons and form negative ions
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15
Q

characteristics of metalloids

A
  • semi malleable/ductile
  • semi-lustrous
  • semiconductors
  • on the metalloid line
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16
Q

define scientific theory

A

a model used to explain how or why a phenomenon occurs

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17
Q

define scientific law

A

a specific statement that is thought to never be violated by the entire natural universe

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18
Q

characteristics of a gas

A
  • no definite shape/volume
  • particles move in random motion with little or no attraction to each other
  • highly compressible
  • MOST chaotic
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19
Q

characteristics of a liquid

A
  • no definite shape
  • definite volume
  • particles are free to move over each other but still attracted to each other
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20
Q

characteristics of a solid

A
  • definite shape/volume
  • particles vibrate around fixed axes
  • least chaotic
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21
Q

Convert 8.025 × 10⁻⁸

A

.00000008025

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22
Q

Convert: 6.924 x 106

A

6,924,000

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23
Q

Convert to Scientific Notation: 156.0

A

1.56 x 10-2

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24
Q

Convert to Scientific Notation:

A

4.8 x 10-4

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25
Q

How many meters are in 57 millimeters

A

.057m

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26
Q
A
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27
Q

Convert 70 miles per hour into meters per second.

A

112653.8 meters/ 1 hour

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28
Q

define density

A

Ratio of substance’s mass to its volume

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29
Q

A cork stopper from a bottle of wine has a mass of 3.78 g. If the density of cork is 0.22 g/cm3, what is the volume of the cork?

A

17.2 cm3

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30
Q

What is the volume of 3.78 g of gold?

A

0.196 cm3

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31
Q

define an atom

A

smallest piece of an element that maintains the identity of that element

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32
Q

define an electron

A

particle with a negative charge, represented as e-
- Location in atom: electron cloud
- Determines: ionic charge

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33
Q

define a proton

A

more massive (but still tiny) particle with a positive charge, represented as p +
- Location in atom: nucleus - Determines: atomic number

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34
Q

define a neutron

A

subatomic particle, same mass as a proton, no charge, represented as n or n0
-Location in atom: nucleus
-Determines: mass number
-Most MASSIVE subatomic particle

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35
Q

define an isotope

A

Atoms of the same element (same # of protons) with different numbers of neutrons

36
Q

How do you know how many isotopes an element has?

A
37
Q

Atomic number =

A

number of protons

37
Q

Element mass # =

A

of protons + # of neutrons

37
Q

Element Charge =

A

of protons - # of electrons

38
Q

What are the diatomic elements?

A

H2, N2, F2, Cl2, Br2, I2

39
Q

What are the greek numerical prefixes?

A

mon (o) - 1
di - 2
tri - 4
tetr(a) - 4
pent (a) - 5
hex (a) - 6
hepta (a) - 7
oct (a) - 8
non(a) - 9
dec(a) - 10

40
Q

define a chemical bond

A

the connection between 2 atoms in a molecule

41
Q

define covalent bonding

A

a compound containing only nonmetals & nonmetals

42
Q

define an ionic bond

A

compound containing both metals & nonmetals

43
Q

Conversion for Celesius to Kelvin

A

K = C + 273

44
Q

Conversion for Celsius to Fahrenheit

A

F = 1.8(C) + 32

45
Q

Conversion Fahrenheit to Celsius

A

C = (F-32)/1.8

46
Q

Which is the lowest temperature?
a. -10 C
b. -15 F
c. 260 K

A

b. -15 F

47
Q

A piece of metal ore weighs 9.25 g. When a student places it into a graduated cylinder containing water, the liquid level rises from 21.25 mL to 26.47 mL. What is the density of the ore?
A) 2.86 g/mL
B) 1.77 g/mL
C) 0.349 g/mL
D) 0.564 g/mL

A

B) 1.77 g/mL

48
Q

Convert the boiling temperature of gold, 2966 degrees Celcius, into degrees Fahrenheit and Kelvin.

A

5371 degrees Fahrenheit
3239 Kelvin

49
Q

Convert the boiling temperature of liquid ammonia, -28.1 degrees Fahrenheit,into Celsius and Kelvin

A

-33.4 degrees Celsius
239.8 K

50
Q

Rules for Pink Naming

A
  • First element in formula is nonmetal/metalloid
  • ONLY for MOLECULES
  • No ions (polyatomic ions)
  • Use Prefixes
  • No swap and drop
51
Q

What are the numeral prefixes?

A

mono - 1
di - 2
tri -3
tetr(a) - 4
pent(a) - 5
hex(a) - 6
hept(a) - 7
oct(a) - 8
non(a) - 9
dec(a) - 10
-leave the a off if followed by an “o” or “a”

52
Q

What are the Roman Numerals?

A

1 = I
2 = II
3 = III
4 = IV
5 = V
6 = VI
7 = VII
8 = VIII
9 = IX
10 = X

53
Q

Name: N2O4

A

dinitrogen tetroxide

54
Q

What do ALL compounds names have in common?

A
  • The end of the second element’s name is changed to “ide”
  • We don’t do this if the second ion is a polyatomic
55
Q

Name: CIF3

A

dinitrogen tetroxide

56
Q

Name: carbon tetrachloride

A

CCL4
carbon = C1 tetrachloride = Cl4

57
Q

Name: diphosphorus pentoxide

A

P2O5
diphosphorus = P2 pentoxide = O5

58
Q

What are the rules for Orange Naming?

A
  • First element in formula is monovalent metal, or 1st is ammonium
  • Metal/amionium + nonmetaln or metal/ammonium + polyatomic ion
  • Ionic compounds NOT molescules
  • NO prefixes or roman nummerals
  • Reduce & Swap + Drop
59
Q

Name: Al2Se3

A

aluminum selenide

60
Q

Name: K3(PO4)

A

potassium phosphate

61
Q

Name: Mg3P2

A

magnesium phosphide

62
Q

Name: SrCl2

A

strontium chloride

63
Q

Name: Ammonium Chloride

A

NH4Cl or (NH4)Cl

64
Q

Name: silver oxide

A

Ag2O

65
Q

Name: Rubidium Sulfide

A

Rb2S

66
Q

Name: Aluminum Nitride

A

AIN

67
Q

What are the rules for Green Naming?

A
  • First element is a multivalent metal
  • metal + nonmetal or metal + polyatomic ion
  • Ionic compounds
68
Q

Steps to Green Naming

A
  1. First element is green
  2. Break the compound into cation and anion (determine charge of both)
  3. Determine names, change end to “-ide”
  4. Use a roman numeral in parentheses to indicate the ionic change of the cation
69
Q

Name: Cr(PO4)2

A

chromium(VI) phosphate

70
Q

Name: SnBr4

A

tin (IV) bromide

71
Q

Name: cobalt(II) carbonate

A

CoCO3

72
Q

Name: lead (II) arsenide

A

Pb3As2

73
Q

Name: copper (II) acetate

A

Cu(C2H3O2)2

74
Q

define atomic mass

A

protons + neutrons in the nucleus
ex: carbon- 12
- mass listed on periodic table

75
Q

Molar mass =

A

Sum of the masses of atoms in a molecule
N2O3 = 76.02

76
Q

Define an Ion

A

electrons move from one atom to another & species with overall electrical charges are formed
Ex: Fe2+

77
Q

Ionic charge: Ca

A

2+

78
Q

Ionic charge: Al

A

3+

79
Q

How do you write ionic formulas?

A
  • the total positive charge must balance the total negative charge
  • has a cation (+) and anion (-)
  • cation is first, anion 2nd
  • swap and drop charges, reduce
80
Q

Ionic formula: Na and Cl

A

NaCl

81
Q

Ionic formula: Mg and Cl

A

MgCl2

82
Q

Rules for writing polyatomic ion compounds

A
  • only ammonium is a cation, the rest are anions
83
Q

Name: NH4+ & S2-

A

Ammonium sulfide

84
Q

Name: Al3+ & PO4 3-

A

Aluminum phosphate

CHEM 120 (3 decks)

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