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10th grade > Chem Final Sem 2 > Flashcards

Chem Final Sem 2 Flashcards

1
Q

Oxidation numbers, what are they?

A

+ or - charge on atom or group of atoms

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2
Q

Give two examples of an element or polyatomic ion with its oxidation number

A

Na+,

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3
Q

List the prefixes in order from 1 through 9

A

1- Mono
2- Di
3- Tri
4- Tetra
5- Penta
6- Hexa
7- Hepta
8- Octa
9- Nona

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3
Q

Greek prefixes – what do they tell us?

A

The number of whatever the item is

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4
Q

Compound naming: you should be able to use your Ion Chart and be able to name binary ionic
compounds!
SbN

A

Antimony (III) Nitride

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5
Q

What does binary mean

A

2 parts

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6
Q

What does ionic mean

A

Atom loses electron to other when they bond

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7
Q

What is cation and which part of formula do you see it

A

Positive ion, in very front

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8
Q

LiH which is cation

A

Li

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9
Q

Formula for sodium benzoate

A

Na2C7H6O2

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10
Q

Formula for magnesium acetate

A

Mg(C2H3O2)2

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11
Q

Formula for Iron (III) chloride and Iron (II) chloride

A

Iron (III) chloride- FeCl3
Iron (II) chloride- FeCl2

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12
Q

What’s the difference between Iron (III) and Iron (II)

A

+2 vs +3 charge (oxidation #)

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13
Q

What is stock system of naming compounds and give examples

A

Iron (II) oxide
Antimony(III) Phosphide

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14
Q

Why is it important to balance the + and - charges of ions in a formula

A

Balances to 0 which is neutral and less likely to react

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15
Q

Water can and does attach itself to the crystalline structure of a molecule. What is the water called?

A

Hydrate

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16
Q

What do we call a compound that has no water in the molecule?

A

Anhydrous

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17
Q

What is the name for MgSO4 * 3H2O

A

Magnesium sulfate Trihydrate

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18
Q

Chemical formula for calcium fluoride

A

CaF2

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19
Q

Chemical formula for silicon disulfide?

A

SiS2

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20
Q

What is the reactant or reactants and product or products in 4Fe + 3O2 —-> 2Fe2O3

A

Reactant: 4Fe + 3O2
Products: 2Fe2O3

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21
Q

Define reactant and product in any chemical equation.

A

Reactant- what starts at beginning (ingredients)
Product- what you get at the end

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22
Q

What are coefficients and subscripts

A

Coefficients- How many of that atom or molecule is in equation
Subscript- How many atoms or group of atoms there are

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23
Q

Coefficients and subscript for 3H2 + O2 —-> 3H2O

A

Coefficients- 3
Subscripts- 2

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24
Q

What part of any equation can we change to balance all the atoms of each element on both sides of the equation?

A

Coefficients only

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25
Q

Why do we need to balance every atom of every element on both sides of reaction

A

Law of mass conservation: you can’t have matter disappear in universe like that

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26
Q

NaCl(s)
(s) means

A

Solid was produced

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27
Q

NaCl(aq)
(aq) means

A

Aquaeous; dissolved in water=solution

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28
Q

N2(g)
(g) means

A

Gas was produced

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29
Q

What does —–> mean

A

Yields or this will result in

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30
Q

What does (triangle sign) above arrow mean

A

Heat was added to get reaction going

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31
Q

When you see an element above arrow, it means it’s catalyst. What do they do

A

Speeds up reaction while its unchanged

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32
Q

Synthesis reaction

A

Make something by combining reactants
2H2 + O2 —-> 2H2O

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33
Q

Decomposition reaction

A

Break down something
CaCl2 —> Ca + Cl2

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34
Q

Single replacement reaction

A

Cations swap places
Mg + CuSO4 —> Cu + MgSO4

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35
Q

Double replacement reaction

A

Cations swap places but no cation is left alone
AgNO3 + NaCl —> AgCl + NaNO3

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36
Q

What do net ionic equations show*

A

Ions that actually react

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37
Q

What are spectator ions*

A

Appears in both reactants and products; it doesn’t react with other ions

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38
Q

Describe what is a mole, what is number value of mole

A

Its a number
6.022 x 10^23 of anything

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39
Q

Mole is also known as __________________

A

Avogandro’s number

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40
Q

What is Avogandro’s number based on

A

12.01 grams per mole of Carbon-12

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41
Q

2 examples of mole used in chem

A

1 mole of Hydrogen atoms weigh 1.01 g

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42
Q

One mole of CO2 contains ___ moles of carbon atoms and ____ moles of oxygen atoms

A

1, 2

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43
Q

Molar mass is typically expressed in which unit?

A

Grams/mole

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44
Q

What type of formula best represents the arrangement of bonds in a molecule?

A

Structural formula

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45
Q

What is the molar mass of carbon monoxide?

A

28 g

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46
Q

Where can you find the information needed to change grams of a substance to moles?

A

Periodic table show you the grams per mole of an element.

47
Q

Limiting reactant

A

Reactant thats used up 1st before other reactants in reaction
Prevents more product from forming

48
Q

Excess reactant

A

Any leftover reactants when reaction is finished

49
Q

Empirical formula

A

Simplest form of a formula . Numbers cannot be divided even lower.
P10H14 no P5H7 yes

50
Q

Molecular formula

A

Shows all the elements and how many of each element in the formula
C2H6O

51
Q

Structural formula

A

Number and types of atoms involved. How these atoms are put together

52
Q

Yield

A

How much product are you getting at the end

53
Q

Actual yield

A

Physically measured amount of of product at end of reaction

54
Q

Theoretical yield

A

Max amnt of product made that is calculated on paper from a given amnt of reactant

55
Q

Percent yield

A

Percentage of theoretical yield that was actually produced

56
Q

The most important indicator of efficiency for a chemical manufacturing company is its ____________ yield

A

Percent

57
Q

Solute vs solvent

A

Solute: Dissolved substances in solution
Colvent: Major part of solution, does dissolving

58
Q

What makes up most of solution

A

Solvent

59
Q

Example of liquid, solid, and gas solution

A

Liquid: Coffee
Solid: Staples
Gas: Atmosphere

60
Q

Properties of solutions

A

Solutes can’t be filtered out of solution
Solutes don’t settle out of solution
Solutions are uniform
Solutions are not chemically combined
Solutions can vary in their concentration

61
Q

How does water dissolve NaCl

A

Solvation

62
Q

Solutions can occur in solids, liquids, and gases. Y/N

A

Yes

63
Q

Can you have more than one solute in solution

A

Yes
Ex: Soda

64
Q

Characteristics of acid and base

A

Acid: Sour, electrolyte, react with metals to product H+ gas and salt, pH below 7
Base: Bitter, feels slippery, some are electrolytes, pH above 7

65
Q

Electrolyte

A

Substance that ionizes to conduct electricity in solution

66
Q

pH means what

A

Power of hydrogen

67
Q

pOH means what

A

Power of hydroxide

68
Q

What is pH and pOH scale based on

A

Ionization constant of water

69
Q

What does pH scale tell you

A

How acidic or basic/alkaline a substance is

70
Q

What does pOH scale tell you

A

Hydroxide ion concentration

71
Q

pH = 7 tells what

A

Neutral solition

72
Q

pH < 7 vs pH > 7

A

pH < 7 = acid
pH > 7 = base

73
Q

pOH < 7 vs pOH > 7

A

pOH < 7 = Base
pOH > 7 = Acid

74
Q

Strong vs weak acid

A

Strong: Give up protons easily, ionize completely, dissolves well
Weak: Don’t dissociate (separate) completely into ions, dissolve poorly in water

75
Q

Strong vs weak base

A

Strong: Accept proton readily, dissolves well
Weak: Weak proton acceptors, doesn’t dissolve well

76
Q

Neutralization, whats the idea

A

Acid and base neutralize each other as they are opposites

77
Q

Acid + base ——-> ____________ + __________

A

Salt, water

78
Q

If you look at a glass of water, are 100% of water in there H2O

A

No

79
Q

Conjugate acid

A

Formed when proton is transformed to the base
Base gains H+ —-> Conj acid

80
Q

Conjugate base

A

Everything that remained of acid molecule after a proton is lost
Acid loses H+ —-> Conj base

81
Q

Bases and acids are they the same or are they ___________________

A

Opposites

82
Q

Oh my lady gaga you spilled base on your arm! How do you respond to neutralize it?

A

Add acid on it

83
Q

Titrations

A

Controlled neutralization reactions that are used to determine unknown concentration of solution

84
Q

Equivalence point

A

Equal moles of acid and base

85
Q

End point

A

Color changes at pH 7

86
Q

MaVa = MbVb tells what

A

Equation used to solve for unknown molarity concentrations

87
Q

Buffer

A

Solutions that resist changes in pH. Most effective at regulating slight pH changes

88
Q

Bronsted-Lowry acid and base

A

Acid donates proton (deprotonation)
Base accepts proton (protonation)

89
Q

What does REDOX mean

A

Oxidation reduction reaction

90
Q

Reduction; give half equation ex

A

Atom gains electron/s
Ex: Na —> Na+ + 1e-

91
Q

Oxidation; give half equation ex

A

Atom loses electron’s
Ex: Na+ + 1e- —> Na

92
Q

What is being lost or gained in any REDOX reaction

A

Electrons

93
Q

Oxidation agents

A

Atoms that would cause another atom to lose electrons

94
Q

Reduction agents

A

Atoms that would cause another atom to gain electrons

95
Q

Weak electrolyte vs strong electrolyte, which is better electrical conductor

A

Strong bc they allow more electrons to conduct

96
Q

Spontaneous

A

No energy needed to get reaction going
Ex: Voltaic/galvanic battery, vinegar reacting w/baking soda

97
Q

Nonspontaneous

A

You need energy to get the reaction going
Ex: Recharging a battery by running electricity and causing chemical reaction to go backwards to charge battery

98
Q

Anode

A

Attracts anions; is positive; oxidation

99
Q

Cathode

A

Attracts cations; negative; reduction

100
Q

RED CAT

A

Reduction cathode- gains electrons from anode

101
Q

AN OX

A

Oxidation anode- Electrons leave to go to cathode

102
Q

Zinc anode

A

Provides electrons to go through circuit, power up what is hooked up and goes on to cathode
As it loses electrons, zinc begins to disintegrate

103
Q

Copper cathode

A

Where all electrons go to accumulate on copper electrode due to electrons attracting copper ions

104
Q

Salt bridge, why do we need it for battery to work

A

Electrochemical cells
Needed to assure neutrality of both compartments

105
Q

Voltaic cell aka galvanic cell

A

Cell that provides electricity to power devices like phone

106
Q

Intermolecular forces types, rate from strongest to weakest

A

Hydrogen bonding
Dipole-dipole
London (Dispersion) forces

107
Q

Intermolecular force that exist btwn only nonpolar molecules (ex: oil) would be

A

London dispersion forces only

108
Q

Why does water have a high boiling point? Why does it exist as a liquid at room temperature

A

Hydrogen bonds make water have higher boiling

109
Q

Of all states of matter: Solid liquid gas and plasma, would you expect it to be the heaviest

A

Solid is heaviest except water due to how many molecules form when frozen

110
Q

Evaporation vs vaporization

A

Both involving changing liquid to gas <— alike
Evaporation is off the surface and below the boiling point.
Vaporization is the surface and happening in the inside of a liquid

111
Q

Which is it, evaporation or vaporization would you expect to occur at the boiling point?

A

Both can happen there but vaporization is the main one because it is a total change.

112
Q

What is the binding forces in crystals forming a crystal lattice , like NaCl, or sugar?

A

(Attractions between molecules)

113
Q

How can we cause a crystal lattice to melt?

A

Add thermal energy. (Heat)

114
Q

Why do crystal lattices melt?

A

Adding thermal energy overcomes the crystal lattice and the solid begins to melt.

10th grade (71 decks)

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