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
Specific heat equation (written)
Specific heat = amount of heat energy/mass × change in temp
26
Specific heat equation (with coefficients)
Cp = Q/m • ∆T ``` Q = m•Cp•∆T ∆T= Tfinal - Tinitial ```
27
``` Specific heat coefficients: Cp= Q= m= ∆T= ```
``` Cp= specific heat Q= amount of heat m= mass ∆T= change in temp ```
28
Specific heat units
J/g • ℃ or cal/g • ℃
29
Specific heat units of water
4.184 × J/g • ℃ = 1.0cal/g • ℃
30
Heat energy units
joule (J) and calorie (cal)
31
1 cal = _ J (exact)
1 cal = 4.184 J
32
Conductors are (metals/nonmetals)
Conductors are metals
33
Conductors have (high/low) specific heat
Conductors have LOW specific heat
34
Non-conductors are (metals/nonmetals)
Non-conductors are nonmetals
35
Non-conductors have (high/low) specific heat
Non-conductors have HIGH specific heat
36
To “burn calories” food is burned in a __ to determine their __
burned in a calorimeter to determine their energy values
37
Burned calorie units
kJ/g or kcal/g
38
Energy values for foods? (3)
kilocalories, kilojoules, and Calorie
39
kilocalories = kilojoules = Calorie=
kilocalories = g • kcal/g kilojoules = g • kJ/g Calorie= kcal
40
1 Cal = _ kcal = _ cal
1 Cal = 1 kcal = 1000 cal
41
1 Cal = _ kJ = _ J
1 Cal = 4.184 kJ = 4184 J
42
Energy values for Carbohydrates: _ kcal/g and _ kJ/g
4 kcal/g and 17 kJ/g
43
Energy values for Fats: _ kcal/g and _ kJ/g
9 kcal/g and 38 kJ/g
44
Energy values for Proteins: _ kcal/g and _ kJ/g
4 kcal/g and 17 kJ/g
45
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
- 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
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
- 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
Properties of metalloids: (6 total) Are _ compared to metals and nonmetals and are are also called _
in between metals and nonmetals “semiconductors”
48
Location of: protons, neutrons and electrons in atom composition
Proton- Nucleus Neutron- Nucleus Electron- Electron Cloud
49
Atomic radius is
a length equal to half the distance between the nuclei of two covalently bonded atoms
50
Ionic radius is
the distance from the nucleus to the outermost e- of an ion | Atomic/ionic radii
51
Cation is a positively charged ion of a metal | Cations are much (smaller/larger)
positively charged ion of a metal | Cations are much smaller
52
Anion is a negatively charged ion | Anions are somewhat (smaller/larger)
Anion is a negatively charged ion | Anions are somewhat larger
53
For ions in the same period (row): More positive = (smaller/larger)
More positive = smaller
54
For ions in the same period (row): More negative = (smaller/larger)
More negative = larger
55
Biological Roles of K+ (4)
- Membrane transport - Neurotransmission - Muscle contraction - Heart function
56
In the body Thallium (I) can...
pretend to be K+ but reacts differently, so you will die quickly and painfully
57
``` Ionic compounds are __ + __ and you (do/don't) reduce to lowest ratio ```
METAL + NONMETAL | REDUCE to lowest ratio
58
Ionic bonding is
the attraction between positive and negative ions in an ionic compound
59
``` Covalent molecules are __ + __ and you (do/don't) reduce to lowest ratio ```
NONMETAL + NONMETAL | DO NOT reduce
60
Covalent bonding
holds the shared atoms together and forms a molecule
61
***Valence electron is | felt smart, might delete later
an electron in an outer shell of an atom that can be lost to or shared with another atom to form a molecule
62
In naming Ionic Compounds, if the first atom is orange = formula unit Indicate charge with a Roman numeral?
Metal only has one possible ion so no need to indicate charge with a Roman numeral
63
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
Al2Se3, ammonium chloride, K(PO4), SrCl2 NOTICE: metal + nonmetal reduced to lowest ratio Roman numeral is NOT used
64
In naming Ionic Compounds, if the first atom is green = formula unit Indicate charge with a Roman numeral?
Metal has many possible ionic charges, use Roman numerals
65
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
Cr(PO4)2, Cobalt (II) carbonate, Lead (II) arsenide, Mn(SO4)7 NOTICE: metal + nonmetal reduced to lowest ratio Roman numeral IS used
66
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
Name the compound with prefixes that refer to the subscripts | DO NOT reduce the subscripts
67
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
SeF6, Sulfur monoxide, N2O4, ClF3, Triboron silicide NOTICE: nonmetal + nonmetal subscripts are NOT reduced Roman numeral is NOT used
68
``` Prefixes for Molecular Compounds: 1. (remember) 2. 3. 4. 5. 6. 7. 8. 9. 10. Remember overall: (a's and o's) ```
``` 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
Writing Molecular Chemical Formulas: Covalent molecules are composed of __, not ions. To write the molecular formula you need to know
Composed of neutral atoms, not ions. The name of the molecule
70
***Empirical formulas
Empirical formulas 
**Need to know element symbols and polyatomic ion/acid formulas**
71
***Empirical formulas | felt smart, might delete later
Empirical formulas 
**Need to know element symbols and polyatomic ion/acid formulas**
72
Metalloid acronym
``` (B) Be (Si) So (Ge) Great (As) Assholes (Sb) Stay (Te) Troubled ```
73
Metalloids (6 total)
``` boron (B) silicon (Si) germanium (Ge) arsenic (As) antimony (Sb) tellurium (Te) ```