Chemistry Test #2

Front 1

Ionic Bonds occur between?

Back 1

1. Metals and Nonmetals
2. Involves TRANSFER of electrons from one atom to another.
3. Metal atom becomes cation, nonmetal becomes anion.

Front 2

Covalent Bonds occur between?

Back 2

1. Two or more nonmetals
2. Involves the SHARING of electrons between atoms.

Front 3

What is the lowest potential energy/most stable state of a covalent bond?

Back 3

1. When the electron is between two protons.

Front 4

Empirical formula represents?

Back 4

1. Elements present and relative number of atoms of ions.
2. Divides by smallest number (C4H8) would be written CH2

Front 5

Molecular formula represents?

Back 5

1. Elements present and ACTUAL number of atoms of each element.

Front 6

Structural formula represents?

Back 6

1. Uses lines to represent covalent bonds, shows how connected.
2. H-O-O-H

Front 7

Ball and stick models show what?

Back 7

1. represent atoms as balls and chemical bonds as sticks.
2. How the two connect represents molecule's shape.

Front 8

Space-filling models show what?

Back 8

1. Atoms fill space between them to more closely represent best estimates on how molecule may appear if scaled to visible size.

Front 9

What is the molecular formula for methane and what shape does it form in the ball and stick model?

Back 9

1. CH4
2. Tetrahedron

Front 10

Why are atomic structures not flat/linear?

Back 10

1. Because there are electrons called nonbonding electrons on the atom which creates an electrical cloud that pushes on the other electrical clouds of the electrons, which forms a non-flat shape.

Front 11

What is the difference between Atomic elements and Molecular elements?

Back 11

1. Atomic elements are those that exist in nature with single atoms as their basic units.
2. Molecular elements are those that exist with two or more atoms bonded together. - Most exist as diatomic molecules. H2, N2, Cl2.
3. A few polyatomic exist: Phosphorous, P4 and Sulfur, S8.

Front 12

Molecular compounds normally are composed of.......

Back 12

1. Two or more covalently bonded NONMETALS.

Front 13

Ionic Compounds are composed of......

Back 13

1. Cations (usually one type of metal) and Anions (usually nonmetal) bound together by ionic bonds.

Front 14

What is a formula unit?

Back 14

1. Smallest, electrically neutral collection of ions.

Front 15

What is a polyatomic ion?

Back 15

1. An ion composed of two or more atoms.

Front 16

Ionic compounds always contain....

Back 16

1. Positive and negative ions.

Front 17

Common names are....

Back 17

1. nicknames, such as (NaCl) table salt, NaHCO3) baking soda.
2. Little info on chemical structure

Front 18

Systematic names are...

Back 18

1. official name of a compound, that can be established by looking at its chemical structure.

Front 19

What metals have more than one cation, so their charge needs to be named in roman numeral?

Back 19

1. Transition metals usually do, but Tin does as well.

Front 20

What are oxyanions?

Back 20

1. Anions containing oxygen and another element.
2. Most polyatomic ions are oxyanions.

Front 21

What is the name of ClO4-
What is the name of ClO -
What is the name of ClO 2-
What is the name of ClO 3 -

Back 21

1. Perchlorate (oxyanion)
2. Hypochlorate (oxyanion)
3. Chlorite
4. Chlorate

Front 22

What do you put in front of molecular compounds?

Back 22

1. Prefixes (mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca)

Front 23

What are hydrates?

Back 23

1. Ionics compounds that contain a specific number of water molecules associated with each formula unit.

Front 24

Acids are...

Back 24

1. molecular compounds that release hydrogen ions (H+) when dissolved in water.
2. They are composed of water and another nonmetal written second.
3. Written as HCl (aq)

Front 25

What is a binary acid versus a oxyacid?

Back 25

1. Binary acid: composed of hydrogen and nonmetal.
2. Hydro - (nonmetal)ic acid.
3. Oxyacid: contain hydrogen and an oxyanion.
4. Oxyanions ending in ate = (oxyanion) ic acid.
5. Oxyanions ending in ite = (oxyanion) ous acid.

Front 26

What is the formula mass?

Back 26

1. Sum of the atomic masses of all the atoms in its chemical formula.
2. Same as molar mass, just measured in AMU not g/mol

Front 27

What is mass percent or mass percent composition?

Back 27

1. Element's percentage of the compound's total mass.
2. Mass % = Mass of element X in 1 mol/mass of 1 mol of whole compound. X 100

Front 28

What is the empirical formula molar mass?

Back 28

1. Sum of all masses of all the atoms in the empirical formula.

Front 29

What is combustion analysis?

Back 29

1. An unknown compound undergoes combustion (burning) in the presence of pure oxygen.
2. All carbon is converted into CO2 and all hydrogen is converted into H2O.
3. The CO2 and H2O are weighed and numerical relationships in mols are used to determine original sample amounts of C and H.

Front 30

What is a chemical reaction?

Back 30

1. process in which one or more substances are converted into one or more different ones.

Front 31

What is a combustion reaction?

Back 31

1. Type of chemical reaction
2. Substance combines with oxygen to form one or more oxygen-containing compounds.
3. Emit heat, useful for energy.
4. IE: gasoline, natural gas heating homes, etc.

Front 32

What is a hydrocarbon?

Back 32

1. Organic compounds that contain only carbon and hydrogen.

Front 33

What are alkanes?

Back 33

1. Hydrocarbons containing only single bonds

Front 34

What is an alkene?

Back 34

1. Hydrocarbon containing double bonds.

Front 35

What is an alkyne?

Back 35

1. Hydrocarbon containing a triple bond.

Front 36

What is a functional group?

Back 36

1. Characteristic atom or group of atoms.

Front 37

Alcohols have a _____ functional group?

Back 37

1. -OH

Front 38

Name each ionic compound..
1. CsF
2. KI
3. SrCl2
4. BaCl2
5. Ba(OH)2
6. NH4I
7. NaBrO4
8. Fe(OH)3
9. CoSO4
10. KClO

Back 38

1. Cesium Flouride
2. Potassium Iodide
3. Strontium Chloride
4. Barium Chloride
5. Barium Hydroxide
6. Ammonium Iodide
7. Sodium Bromate
8. Iron (III) Hydroxide
9. Cobalt (II) Sulfate
10. Potassium Hypochlorite

Front 39

Write formula for each ionic compound...
1. Copper (II) Chloride
2. Copper (I) Iodate
3. Lead (II) Chromate
4. Calcium Flouride
5. Potassium Hydroxide
6. Iron (II) Phosphate

Back 39

1. CuCl2
2. CuIO3
3. PbCrO4
4. CaF2
5. KOH
6. Fe3(PO4)2

Front 40

Name each molecular compound...
1. SO3
2. SO2
3. BrF5
4. NO
5. XeO3

Back 40

1. Sulfer Trioxide
2. Sulfer Dioxide
3. Bromine Pentaflouride
4. Nitrogen Monoxide
5. Xenon Trioxide

Front 41

Write a formula for each molecular compound...
1. Boron Tribromide
2. Dichlorine Monoxide
3. Xenon Tetraflouride
4. Carbon Tetrabromide
5. Diboron Tetrachloride

Back 41

1. BBr3
2. Cl2O
3. XeF4
4. CBr4
5. B2Cl4

Front 42

Write formula for each acid...
1. Phosphoric acid
2. Hydrocyanic acid
3. Chlorous acid

Back 42

1. H3PO4 (aq)
2. HCN (aq)
3. HClO2 (aq)

Front 43

Calculate the formula mass for each compound...
1. MgBr2
2. HNO2
3. CBr4
4. Ca(NO2)2

Back 43

1. 184.11 g
2. 47 g
3. 331.6 g
4. 132 g

Front 44

Determine amount of moles of oxygen in each sample.
1. 4.88 mole H2O2
2. 2.15 mol N2O
3. .0237 mol H2CO3
4. 24.1 mol CO2

Back 44

1. 9.76 mol
2. 2.15 mol
3. .0711 mol
4. 48.2 mol

Front 45

Calculate the mass percent composition of nitrogen in each compound...
1. N2O
2. NO
3. NO2
4. HNO3

Back 45

1. 63 %
2. 46 %
3. 30 %
4. 22 %

Front 46

Calculate the mass of each sample...
1. 15.7 mol HNO3
2. 1.04 X10-3 mol H2O2
3. 72.1 mol SO2
4. 1.23 mol Xenon Diflouride

Back 46

1. 989.1 g
2. .03536 g
3. 4619.5 g
4. 208.22 g

Front 47

Calculate empirical formula for each decomp reaction...
1. 1.245 g Ni, 5.381 g I
2. 2.677 g Ba, 3.115 g Br
3. 2.128 g Be, 7.557 g S, 15.107 g O

Back 47

1. NiI2
2. BaBr2
3. Be2S2O

Front 48

Calculate empirical formula from mass percentage... (set equal to 100 gram sample)
1. C 58.8 %, H 9.87 %, O 31.33 %
2. C 63.15 %, H 5.30 %, O 31.55 %

Back 48

1. C5H10O2
2. C5H5O2

Front 49

What is a binary compound?

Back 49

1. Compound with just two elements.

Front 50

Stoichiometry...

Back 50

1. Numerical relationship between chemical amounts in a balanced chemical equation.

Front 51

Limiting reactant...

Back 51

1. Reactant that limits the amount of product in a chemical reaction.
2. Find reactant with least amount of moles.

Front 52

Theoretical yield...

Back 52

1. Amount of product that can be made in a chemical reaction based on the amount of limiting reactant.

Front 53

Percent yield...

Back 53

1. Actual yield/theoretical yield X100

Front 54

Solvent...

Back 54

1. Something dissolves into it.
2. Water

Front 55

Solute...

Back 55

1. Something that dissolves in water or other solution.
2. Sugar

Front 56

Dilute solution...

Back 56

1. One that contains a small amount of solute (sugar) relative to the solvent. (water)

Front 57

Concentrated solution...

Back 57

1. One that contains a large amount of solute (sugar) relative to solvent (water).

Front 58

Molarity...

Back 58

1. Amount of solute (mol)/volume of solution (L)
2. Mol/Liters

Front 59

Stock solution...

Back 59

1. Concentrated forms of a solution.

Front 60

Electrolytes...what and are they ionic or molecular compounds?

Back 60

1. Substances that dissolve in water to form solutions that conduct electricity.
2. Salt solution
3. USUALLY IONIC COMPOUNDS.

Front 61

Strong electrolytes...

Back 61

1. Substances such as sodium chloride that completely dissociate into ions when they dissolve in water.

Front 62

Non-electrolytes...

Back 62

1. Compounds such as sugar that do not dissociate into ions when dissolved in water.
2. MOLECULAR COMPOUNDS such as sugar
3. DO NOT CONDUCT ELECTRICITY.

Front 63

Strong Acid...

Back 63

1. One that completely ionizes in a solution.
2. HCL
3. Strong acid = strong electrolyte

Front 64

Weak acid...

Back 64

1. Do not completely ionize in water.
2. Weak acids = weak electrolytes - conduct electricity weakly.

Front 65

Soluble vs. Insoluble

Back 65

1. Soluble = Dissolves in water
2. Insoluble = does NOT dissolve in water.
3. Although some have a small degree of solubility even if insoluble.

Front 66

What are precipitation reactions?

Back 66

1. Ones in which a solid or precipitate forms upon mixing two solutions.
2. Taking bath with hard water, scum forms.
3. ONLY INSOLUBLE PRODUCTS PRODUCE SOLIDS.

Front 67

Molecular equation...

Back 67

1. An equation showing the complete neutral formulas for each compound in the reaction as if they existed as molecules.
2. Although they are usually present as ions.

Front 68

Complete ionic equations...

Back 68

1. Equations that list all of the ions present as either reactants or products in a chemical reaction.

Front 69

Spectator ions...

Back 69

1. Ions in solutions that don't change on both sides of reaction.

Front 70

Net Ionic equations...

Back 70

1. Only show species that actually change during reaction.

Front 71

Acid-base reactions...

Back 71

1. Also called neutralization reaction.
2. An acid reacts with a base and the two neutralize each other, producing WATER.

Front 72

Gas-Evolution reaction...

Back 72

1. Gas forms, resulting in bubbles.
2. Many are also acid-base reactions.
3. Anion combines with Cation of another element.

Front 73

What does an acid produce in aq?

Back 73

1. H+ ions

Front 74

What does a base produce in aq?

Back 74

1. OH- ions

Front 75

What are polyprotic acids?

Back 75

1. contain more than one ionizable proton and release them sequentially.

Front 76

Diprotic acid?

Back 76

1. H2SO4
2. Releases first H+ as it is strong, then the second time it is weak and releases its second H+ ion.

Front 77

What is a titration?

Back 77

1. Substance in a solution of known concentration is reacted with another substance in a solution of unknown concentration.

Front 78

Equivalence point??

Back 78

1. Point in titration when number of moles of OH- equals number of H+ moles in solution.
2. Pronouced by indicater, usually dye.

Front 79

Redox reactions (oxidation-reduction)

Back 79

1. reactions in which electrons are transferred from one reactant to the other.

Front 80

Oxidation vs. Reduction?

Back 80

1. Oxidation lose electrons
2. Reduction gains electrons
OIL RIG - Oxidation is loss, reduction is gain.

Front 81

Oxidation number of atom?

Back 81

1. the "charge" it would have if all shared electrons were assigned to the atom with greater attraction for these electrons.
2. Usually charge.
3. Must be multiplied by number of atoms H2O, 2(ox state H), (ox state O)
4. O -1, H +1, Group 1 and 2 are normal charge, etc.

Front 82

What is a hydronium ion?

Back 82

1. H3O+
2. ion formed from association of a water molecule with an H+ ion donated by acid.

Front 83

Family?

Back 83

1. Group of organic compounds with the same functional group.

Front 84

Solution...

Back 84

1. Homogeneous mixture of two substances - such as salt and water.