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CHEM 120 SUMR'DONE > Unit 1: Chapters 1-4 > Flashcards

Unit 1: Chapters 1-4 Flashcards

1
Q

Density equation

A

D= m/v

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2
Q

Specific gravity equation

Units?

A

S.G. = Dsolute/DH2O

NO UNITS

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3
Q

High specific gravity has large quantities of proteins in (solutes/solvent-water) than (solutes/solvent-water)

A

in solutes-salts/sugar/proteins than solvent-water

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4
Q

Low specific gravity has much more (solutes/solvent-water) than (solutes/solvent-water)

A

much more solvent-water than solutes-salts/sugar/proteins

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5
Q

Low specific gravity is close to __’s density

A

water’s density

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6
Q

Elements are __ substances

A

pure substances

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7
Q

Compounds are __ substances

A

pure substances

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8
Q

Mixtures are a __ combination

A

physical combination

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9
Q

Homogeneous mixtures are

A

mixed so well you CANNOT distinguish the different components visually

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10
Q

In heterogeneous mixtures you (can/can’t) …

A

you CAN distinguish the components but may need a microscope

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11
Q

Heterogeneous mixture examples

A

blood, milk

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12
Q

Physical properties are

A

properties that can be observed WITHOUT changing the identity of the substance under observation

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13
Q

Physical property examples

A

temp at which a substance changes state (boiled water is still water), size, malleability, conductivity, density, etc.

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14
Q

Chemical properties can only be observed…

A

DURING a change in the identity of the substance under observation

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15
Q

Chemical property examples

A

a chemical might be corrosive, combustible, explosive, etc.

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16
Q

Physical change is

A

a process that does NOT change the identity of the substance under observation (just a change in physical state)

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17
Q

Physical change examples

A

melting, boiling, grinding, etc.

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18
Q

Chemical change is

A

a process that DOES change the identity of the substance under observation

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19
Q

The formation of a new compound in chemical changes are also called

A

Reactions

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20
Q

Chemical change examples

A

rusting, tarnishing, burning, etc.

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21
Q

Temperature equation for ℃ and ℉

A

5F= 9C+160

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22
Q

Temperature equation(s) for ℃ and K

A 
K-273= C
C+273= K
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23
Q

Absolute zero= _ K

K (is/isn’t equal to) negative values

A

Absolute zero= 0 K

K ≠ negative values

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24
Q

Specific heat definition

A

the amount of heat required to raise the temperature of 1 gram of a substance 1℃

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25
Q

Specific heat equation (written)

A

Specific heat = amount of heat energy/mass × change in temp

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26
Q

Specific heat equation (with coefficients)

A

Cp = Q/m • ∆T

Q = m•Cp•∆T
∆T= Tfinal - Tinitial
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27
Q 
Specific heat coefficients:
Cp=
Q=
m=
∆T=
A 
Cp= specific heat
Q= amount of heat
m= mass
∆T= change in temp
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28
Q

Specific heat units

A

J/g • ℃ or cal/g • ℃

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29
Q

Specific heat units of water

A

4.184 × J/g • ℃ = 1.0cal/g • ℃

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30
Q

Heat energy units

A

joule (J) and calorie (cal)

31
Q

1 cal = _ J (exact)

A

1 cal = 4.184 J

32
Q

Conductors are (metals/nonmetals)

A

Conductors are metals

33
Q

Conductors have (high/low) specific heat

A

Conductors have LOW specific heat

34
Q

Non-conductors are (metals/nonmetals)

A

Non-conductors are nonmetals

35
Q

Non-conductors have (high/low) specific heat

A

Non-conductors have HIGH specific heat

36
Q

To “burn calories” food is burned in a __ to determine their __

A

burned in a calorimeter to determine their energy values

37
Q

Burned calorie units

A

kJ/g or kcal/g

38
Q

Energy values for foods? (3)

A

kilocalories, kilojoules, and Calorie

39
Q

kilocalories =
kilojoules =
Calorie=

A

kilocalories = g • kcal/g kilojoules = g • kJ/g Calorie= kcal

40
Q

1 Cal = _ kcal = _ cal

A

1 Cal = 1 kcal = 1000 cal

41
Q

1 Cal = _ kJ = _ J

A

1 Cal = 4.184 kJ = 4184 J

42
Q

Energy values for Carbohydrates: _ kcal/g and _ kJ/g

A

4 kcal/g and 17 kJ/g

43
Q

Energy values for Fats: _ kcal/g and _ kJ/g

A

9 kcal/g and 38 kJ/g

44
Q

Energy values for Proteins: _ kcal/g and _ kJ/g

A

4 kcal/g and 17 kJ/g

45
Q

Properties of metals:

  • (Physical state) at room temperature (except __)
  • Highly _
  • Malleable? (can be beaten into sheet/foil)
  • Ductile? (can be drawn into wire)
  • Most have (high/low) densities and melting points
  • Tend to (gain/lose) electrons and form (positive/negative) ions
A
  • Solid at room temperature (except Mercury)
  • Highly lustrous/shiny
  • Malleable, yes
  • Ductile, yes
  • Most have high densities and melting points
  • Tend to lose electrons and form positive ions
46
Q

Properties of nonmetals:

  • (Physical state) with relatively (high/low) melting/boiling points
  • Many properties are _ of metals (examples?)
  • Tend to (gain/lose) electrons and form (positive/negative) ions
A
  • S, L, or G with relatively low melting/boiling points (compared to metals)
  • opposite of metals (e.g. brittle, dull, insulating (non-conductive)
  • Tend to gain electrons and form negative ions
47
Q

Properties of metalloids: (6 total)
Are _ compared to metals and nonmetals
and are are also called _

A

in between metals and nonmetals

“semiconductors”

48
Q

Location of: protons, neutrons and electrons in atom composition

A

Proton- Nucleus
Neutron- Nucleus
Electron- Electron Cloud

49
Q

Atomic radius is

A

a length equal to half the distance between the nuclei of two covalently bonded atoms

50
Q

Ionic radius is

A

the distance from the nucleus to the outermost e- of an ion

Atomic/ionic radii

51
Q

Cation is a positively charged ion of a metal

Cations are much (smaller/larger)

A

positively charged ion of a metal

Cations are much smaller

52
Q

Anion is a negatively charged ion

Anions are somewhat (smaller/larger)

A

Anion is a negatively charged ion

Anions are somewhat larger

53
Q

For ions in the same period (row): More positive = (smaller/larger)

A

More positive = smaller

54
Q

For ions in the same period (row): More negative = (smaller/larger)

A

More negative = larger

55
Q

Biological Roles of K+ (4)

A
  • Membrane transport
  • Neurotransmission
  • Muscle contraction
  • Heart function
56
Q

In the body Thallium (I) can…

A

pretend to be K+ but reacts differently, so you will die quickly and painfully

57
Q 
Ionic compounds are \_\_ + \_\_
and you (do/don't) reduce to lowest ratio
A

METAL + NONMETAL

REDUCE to lowest ratio

58
Q

Ionic bonding is

A

the attraction between positive and negative ions in an ionic compound

59
Q 
Covalent molecules are \_\_ + \_\_
and you (do/don't) reduce to lowest ratio
A

NONMETAL + NONMETAL

DO NOT reduce

60
Q

Covalent bonding

A

holds the shared atoms together and forms a molecule

61
Q

***Valence electron is

felt smart, might delete later

A

an electron in an outer shell of an atom that can be lost to or shared with another atom to form a molecule

62
Q

In naming Ionic Compounds, if the first atom is orange = formula unit
Indicate charge with a Roman numeral?

A

Metal only has one possible ion so no need to indicate charge with a Roman numeral

63
Q

Examples of ionic compounds with orange atom first

NOTICE:

  • Types of elements (__ + __)
  • (Is/is not) reduced to lowest ratio
  • Roman numeral (is/is not) used
A

Al2Se3, ammonium chloride, K(PO4), SrCl2

NOTICE:
metal + nonmetal
reduced to lowest ratio
Roman numeral is NOT used

64
Q

In naming Ionic Compounds, if the first atom is green = formula unit
Indicate charge with a Roman numeral?

A

Metal has many possible ionic charges, use Roman numerals

65
Q

Examples of ionic compounds with green atom first

NOTICE:

  • Types of elements (__ + __)
  • (Is/is not) reduced to lowest ratio
  • Roman numeral (is/is not) used
A

Cr(PO4)2, Cobalt (II) carbonate, Lead (II) arsenide, Mn(SO4)7

NOTICE:
metal + nonmetal
reduced to lowest ratio
Roman numeral IS used

66
Q

In naming Molecular Compounds, if the first atom is pink = formula unit
Name the compound with __ that refer to the __
(Do/don’t) reduce the subscripts

A

Name the compound with prefixes that refer to the subscripts

DO NOT reduce the subscripts

67
Q

Examples of molecular compounds with pink atom first

NOTICE:

  • Types of elements (__ + __)
  • Subscripts (are/are not) reduced to lowest ratio
  • Roman numeral (is/is not) used
A

SeF6, Sulfur monoxide, N2O4, ClF3, Triboron silicide

NOTICE:
nonmetal + nonmetal
subscripts are NOT reduced
Roman numeral is NOT used

68
Q 
Prefixes for Molecular Compounds:
1. (remember)
2.
3.
4.
5.
6.
7.
8.
9.
10.
Remember overall: (a's and o's)
A 
mono- (not used on 1st element in a molecule)
di-
tri-
tetr(a)-
pent(a)-
hex(a)-
hept(a)-
oct(a)-
non(a)-
dec(a)-
Remember: ;eave the “a” off it it’s followed by an “o” or “a”
69
Q

Writing Molecular Chemical Formulas:
Covalent molecules are composed of __, not ions.
To write the molecular formula you need to know

A

Composed of neutral atoms, not ions.

The name of the molecule

70
Q

***Empirical formulas

A

Empirical formulas 
Need to know element symbols and polyatomic ion/acid formulas

71
Q

***Empirical formulas

felt smart, might delete later

A

Empirical formulas 
Need to know element symbols and polyatomic ion/acid formulas

72
Q

Metalloid acronym

A 
(B) Be
(Si) So
(Ge) Great
(As) Assholes
(Sb) Stay
(Te) Troubled
73
Q

Metalloids (6 total)

A 
boron (B)
silicon (Si)
germanium (Ge)
arsenic (As)
antimony (Sb)
tellurium (Te)

CHEM 120 SUMR'DONE (9 decks)

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