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CHEM 151 > CHEM Test 2 > Flashcards

CHEM Test 2 Flashcards

1
Q

Metalloids/Semimetals

A

B, Si, Ge, As, Sb, Te

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2
Q

Nonmetals

A

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

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3
Q

Main Group Metals

A

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

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4
Q

Groups

A

Columns of the periodic table

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5
Q

Periods

A

Rows of the periodic table

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6
Q

Covalent bonds

A

non-metal to non-metal

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7
Q

Ionic bonds

A

non-metal to metal

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8
Q

Group 1A

A

alkali metals

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9
Q

Group 2A

A

alkaline earth metals

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10
Q

Group 5A

A

pnictogens

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11
Q

Group 6A

A

chalcogens

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12
Q

Group 7A

A

halogens

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13
Q

Group 8A

A

noble gases

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14
Q

Diatomic elements

A

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

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15
Q

mass spectrometer (long explanation)

A

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.

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16
Q

What does a mass spectrometer do?

A

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.

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17
Q

allotropes

A

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

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18
Q

anhydrous

A

without water

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19
Q

molecular formula

A

describes the composition of molecules ex: C2H6O for Ethanol

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20
Q

condensed formula

A

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

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21
Q

structural formula

A

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.

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22
Q

Strong Acids

A

HCl, HBr, HI, HNO3, H2SO4, HClO4

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23
Q

Strong Bases

A

Anything that contains OH and S

24
Q

Weak Bases

A

NH3, HCO3, CO3

25
Q

Strong Electrolytes =

A

Strong bases, strong acids and soluble salts

26
Q

Weak electrolytes=

A

Weak bases, weak acids and insoluble/sparingly soluble salts

27
Q

solute

A

the stubstance dissolved in a solvent to form a solution

28
Q

solution

A

A homogeneous mixture in a single phase

29
Q

solvent

A

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

30
Q

saturated solution

A

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

31
Q

aqueous solution

A

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

32
Q

Acid definition (Arrhenius)

A

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

33
Q

Acid definition (Lowry/Bronsted)

A

Acid is a proton (H+) donor…
“just add water” making the
hydronium ion H3O

34
Q

formula unit

A

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.

35
Q

empirical formula

A

basic ratio of atoms/moles in a formula

36
Q

oxidized carbon and hydrogen give:

A

H2O and CO2

(but you still need to balance the equation)

37
Q

bases

A

are proton acceptors

38
Q

acids

A

are proton donors

39
Q

carbonates/bicarbonates

(gas-forming reaction)

A

H2CO3

always breaks up and gives H2O and CO2

40
Q

sulfide/bisulfide

A

produces H2S

41
Q

sulfites/bisulfites

A

produces H2SO3

which breaks up into H2O and SO2

42
Q

ammonium salt + OH

A

produces H2O + NH3

43
Q

What are the 4 types of reaction patterns?

A
  1. single displacement
  2. double displacement
  3. synthesis
  4. decomposition
44
Q

What are the 4 types of reactions?

A
  1. acid-base
  2. gas-forming
  3. precipitation
  4. redox
45
Q

What are the 4 types of gas-forming reactions?

A
  1. sulfide/bisulfide (H2S)
  2. carbonate/bicarbonate (H2CO3)
  3. sulfite/bisulfite (H2SO3)
  4. ammonium salt + OH (NH4OH* no such thing)*
46
Q

Oxidation/ Reduction

A

Oxidation – Reducing agent (increased charge)

Is

Loss

Reduction – Oxidizing agent (decreased charge)

Is

Gain

47
Q

Non-Metal Oxides

A

are acidic

48
Q

Metal Oxides

A

are basic

49
Q

Base (Arrhenius definition)

A

increases OH- in a solution

50
Q

Base (Lowry/Bronsted definition)

A

is a proton acceptor

51
Q

Which hydrocarbons are insoluble?

A

The ones that do not contain Oxygen.

52
Q

Which hydrocarbon compounds are soluble?

A

The ones that contain Oxygen.

53
Q

molar mass

A

g/mol

54
Q

molecular mass

A

AMU

55
Q

supersaturated solution

A

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

CHEM 151 (3 decks)

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