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Flashcards

1
Q

well defined repeating patterns, long range order

A

Crystalline solid

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2
Q

order only over very short distance

A

Amorphous solid

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3
Q

how much of an atom is inside when its on a corner

A

1/8

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4
Q

how much of an atom is inside when its on a edge

A

1/4

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5
Q

how much of an atom is inside when its on a face

A

1/2

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6
Q

of nearest neighboring atoms bound to a reference atom

A

Coordination number

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7
Q

nothing in the middle, type of cube, CN= 6, 1 full atom inside, 52% packing efficiency

A

Simple cubic

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8
Q

at corners and 1 in middle, CN=8, 2 atoms total inside, 68% packing efficiency

A

Body centered cube

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9
Q

at corners and 6 faces, CN=12, 4 atoms total inside, 74% packing

A

Face centered cubic

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10
Q

how many atoms inside simple cubic? coordination number?

A

1 atom
CN= 6

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11
Q

how many atoms inside body centered cubic? coordination number?

A

2 atoms
CN= 8

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12
Q

how many atoms inside face centered cubic? coordination number?

A

4 atoms
CN=12

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13
Q

M, moles of solute/ 1 liter of solution

A

Molarity

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14
Q

grams of solute/ 100 grams of solution x 100%

A

Percent by mass

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15
Q

mL of solute/ 100 mL of solution x 100%

A

Percent by volume

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16
Q

higher amount is mixed with solute

A

Solvent

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17
Q

lesser amount is mixed with solute

A

Solute

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18
Q

maximum amount of solute is dissolved

A

Saturated

19
Q

more solute is able to dissolve

A

Unsaturated

20
Q

more than the max is dissolved, usually with heat, causes precipitate

A

Supersaturated

21
Q

why do things mix?

A

because the energy released when a solution is formed (from solute and solvent) is GREATER than the energy required to separate the solute and solvent from themselves

22
Q

soluble or miscible covalent compound

A

Nonelectrolyte

23
Q

slightly soluble ionic compound, weak acid or base

A

Weak electrolyte

24
Q

soluble ionic compound, strong acid or base

A

Strong electrolyte

25
Q

soluble (M)

A

[solute] > 0.1M

26
Q

slightly soluble (M)

A

[solute] btwn 0.01 and 0.1

27
Q

insoluble (M)

A

[solute] < 0.01M

28
Q

make ions in solution and can conduct electricity

A

Electrolytes

29
Q

6 strong acids

A

HCl, HBr, HI, HNO3, H2SO4, HClO4

30
Q

diprotic, triprotic acids are broken down in ____

A

steps:
H3PO4 -> H+ + H2PO4-
H2PO4- ->H+ +HPO42-
HPO4- -> H+ + PO43-

31
Q

solubility rules

A
  1. Compounds of NH4+ and Group 1A are always soluble
  2. NO3-, ClO4-, ClO3- and C2H3O2- are always soluble
  3. Cl-, Br-and I- are soluble except with Ag+, Cu+, TI+, Hg2+ and Pb2+
  4. SO42- is soluble except with Ca2+, Sr2+, Ba2+, and Pb2+
  5. Most other ionic compounds are insoluble and for precipitates
32
Q

Ionic compounds are soluble when q1 and q2 are ____ (charges) and r is _____ (diluted): Coulombs Law

A

small; big

33
Q

actual chemical reaction that occurs without spectator ions

A

Net ionic equations

34
Q

Dilution equation

A

M1V1=M2V2

35
Q

Mass percent= [(moles of element in formula)(molar mass)/molar mass of compound] x 100

A

Mass percent

36
Q

Theoretical yield

A

calculated

37
Q

actual yield

A

experimental

38
Q

percent yield

A

actual/theoretical x 100

38
Q

When 2 liquids mix

A

Miscible

39
Q

Name the parts of a micelle

A

Nonpolar (hydrophobic) interior (tail) with a polar head

40
Q

T/F only ionic compounds can form crystalline solids

A

False

41
Q

Which solutions have the highest conductivities?

A

The ones that dissociate into the most number of ions

42
Q

Which are smaller, cations or anions?

A

Cations

From Flashcardlet (20 decks)

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