CHEM Test 2

Question 1

Metalloids/Semimetals

Answer 1

B, Si, Ge, As, Sb, Te

Question 2

Nonmetals

Answer 2

H, He, C, N, O, F, Ne, P, S, Cl, Ar, Se, Br, Kr, I, Xe, At, Rn

Question 3

Main Group Metals

Answer 3

Li, Na, K, Rb, Cs, Fr, Be, Mg, Ca, Sr, Ba, Ra

Question 4

Groups

Answer 4

Columns of the periodic table

Question 5

Periods

Answer 5

Rows of the periodic table

Question 6

Covalent bonds

Answer 6

non-metal to non-metal

Question 7

Ionic bonds

Answer 7

non-metal to metal

Question 8

Group 1A

Answer 8

alkali metals

Question 9

Group 2A

Answer 9

alkaline earth metals

Question 10

Group 5A

Answer 10

pnictogens

Question 11

Group 6A

Answer 11

chalcogens

Question 12

Group 7A

Answer 12

halogens

Question 13

Group 8A

Answer 13

noble gases

Question 14

Diatomic elements

Answer 14

Bromine, Iodine, Nitrogen, Chlorine, Hydrogen, Oxygen, Fluorine

Question 15

mass spectrometer (long explanation)

Answer 15

Contains an electron beam where high energy electrons collide with the gas phase molecules. Those high energy collisions cause the molecule to lose electrons and turn the molecules into positive ions. These ions usually break apart or fragment into smaller pieces.

Question 16

What does a mass spectrometer do?

Answer 16

A mass spectrometer detects and records the masses of the different particles. Analysis of the spectrum can help identify a compound and can give an accurate molar mass.

Question 17

allotropes

Answer 17

(nonmetals) exist in several different and distinct forms called allotropes, each having its own properties. Carbon has many allotropes (like graphite and diamond)

Question 18

anhydrous

Answer 18

without water

Question 19

molecular formula

Answer 19

describes the composition of molecules ex: C₂H₆O for Ethanol

Question 20

condensed formula

Answer 20

Indicates how certain atoms are grouped together. For example, the condensed formula for ethanol is CH₃CH₂OH

Question 21

structural formula

Answer 21

gives an even higher level of structural detail, showing how all of the atoms are attached within a molecule. The lines between atoms represent the chemical bonds that hold atoms together in this molecule.

Question 22

Strong Acids

Answer 22

HCl, HBr, HI, HNO₃, H₂SO₄, HClO₄

Question 23

Strong Bases

Answer 23

Anything that contains OH and S

Question 24

Weak Bases

Answer 24

NH₃, HCO₃, CO₃

Question 25

Strong Electrolytes =

Answer 25

Strong bases, strong acids and soluble salts

Question 26

Weak electrolytes=

Answer 26

Weak bases, weak acids and insoluble/sparingly soluble salts

Question 27

solute

Answer 27

the stubstance dissolved in a solvent to form a solution

Question 28

solution

Answer 28

A homogeneous mixture in a single phase

Question 29

solvent

Answer 29

The medium in which a solute is dissolved to form a solution

Question 30

saturated solution

Answer 30

When the solution is saturated, the solvent has dissolved the maximum amount of solute that it can at the given temperature.

Question 31

aqueous solution

Answer 31

An aqueous solution is a solution in which the solvent is water.

Question 32

Acid definition (Arrhenius)

Answer 32

Acids increase H⁺/protons in a solution; acids split up and make hydrogen ions.

Question 33

Acid definition (Lowry/Bronsted)

Answer 33

Acid is a proton (H⁺) donor... "just add water" making the hydronium ion H₃O

Question 34

formula unit

Answer 34

A formula unit in chemistry is the empirical formula of any ionic or covalent network solid compound used as an independent entity for stoichiometric calculations. It is the lowest whole number ratio of ions represented in an ionic compound.

Question 35

empirical formula

Answer 35

basic ratio of atoms/moles in a formula

Question 36

oxidized carbon and hydrogen give:

Answer 36

H₂O and CO₂ (but you still need to balance the equation)

Question 37

bases

Answer 37

are proton acceptors

Question 38

acids

Answer 38

are proton donors

Question 39

carbonates/bicarbonates | (gas-forming reaction)

Answer 39

H₂CO₃ always breaks up and gives H₂O and CO₂

Question 40

sulfide/bisulfide

Answer 40

produces H₂S

Question 41

sulfites/bisulfites

Answer 41

produces H₂SO₃ which breaks up into H₂O and SO₂

Question 42

ammonium salt + OH

Answer 42

produces H₂O + NH₃

Question 43

What are the 4 types of reaction patterns?

Answer 43

1. single displacement 2. double displacement 3. synthesis 4. decomposition

Question 44

What are the 4 types of reactions?

Answer 44

1. acid-base 2. gas-forming 3. precipitation 4. redox

Question 45

What are the 4 types of gas-forming reactions?

Answer 45

1. sulfide/bisulfide (H₂S) 2. carbonate/bicarbonate (H₂CO₃) 3. sulfite/bisulfite (H₂SO₃) 4. ammonium salt + OH (NH₄OH* no such thing)*

Question 46

Oxidation/ Reduction

Answer 46

Oxidation -- Reducing agent (increased charge) Is Loss Reduction -- Oxidizing agent (decreased charge) Is Gain

Question 47

Non-Metal Oxides

Answer 47

are acidic

Question 48

Metal Oxides

Answer 48

are basic

Question 49

Base (Arrhenius definition)

Answer 49

increases OH^- in a solution

Question 50

Base (Lowry/Bronsted definition)

Answer 50

is a proton acceptor

Question 51

Which hydrocarbons are insoluble?

Answer 51

The ones that do not contain Oxygen.

Question 52

Which hydrocarbon compounds are soluble?

Answer 52

The ones that contain Oxygen.

Question 53

molar mass

Answer 53

g/mol

Question 54

molecular mass

Answer 54

AMU

Question 55

supersaturated solution

Answer 55

A solution that contains a higher than saturation concentration of solute; therefore, a supersaturated solution is metastable.