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Freshman (semester 1) > Test 2 Chemistry 116 > Flashcards

Test 2 Chemistry 116 Flashcards

1
Q

Covalent compounds are formed between two ___.

A

Nonmetals

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2
Q

Prefixes for binary covalent compounds are:

A

mono-1
di-2
tri-3
tetra-4
penta-5
hexa-6
hepta-7
octa-8
nona-9
deca-10

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3
Q

CO

A

carbon monoxide

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4
Q

SF4

A

sulfur tetrafluoride

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5
Q

Calcium hydride

A

CaH2 (ionic bond haha)

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6
Q

Binary Acids
___ is listed first in the formula
__+nonmetal

A

Hydrogen, H+nonmetal

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7
Q

HF

A

hydrofluoric acid

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8
Q

HCl

A

hydrochloric acid

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9
Q

HBr

A

hydrobromic acid

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10
Q

Oxyacids
__ + polyatomic anion
you can have more than one __ listed first in formula

A

H+polyatomic anion, Hydrogen

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11
Q

ite —> ___
ate –> __
ide —> ___+___

A

ite to ous
ate to ic
ide to hydro ___ ic

HOW TO REMEMBER
my r(IDE) has (HYDRO)lics
i (ATE) something (IC)ky
spr(ITE) is delici(OUS)

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12
Q

SO3, name and charge

A

sulfite, 2-

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13
Q

ClO4, name and charge

A

perchlorate, 1-

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14
Q

ClO, name and charge

A

hypochlorite, 1-

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15
Q

NO3, name and charge

A

nitrate, 1-

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16
Q

NO2, name and charge

A

nitrite, 1-

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17
Q

C2H3O2, name and charge

A

acetate, 1-

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18
Q

PO4, name and charge

A

phosphate, 3-

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19
Q

CO3, name and charge

A

carbonate, 2-

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20
Q

HCN

A

hydrocyanic acid

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21
Q

H3PO4

A

phosphoric acid

22
Q

H3PO3

A

phosphorous acid

23
Q

H2SO4

A

sulfuric acid

24
Q

H2SO3

A

sulfurous acid

25
Q

H3BO3

A

boric acid

26
Q

What are the 7 strong acids

A

HCl —> hydrochloric acid
HBr —> hydrobromic acid
HI —> hydroiodic acid
HClO3 —> chloric acid
HClO4 —> perchloric acid
H2SO4 —> sulfuric acid
HNO3 —> nitric acid

27
Q

Linear Alkane formula

A

C (x) H (2x+2)

28
Q

Linear Alkane prefixes

A

meth-1
eth-2
prop-3
but-4
pent-5
hex-6
hept-7
oct-8
non-9
dec-10

29
Q

NH2

A

amino group

30
Q

COOH

A

carboxylic group

31
Q

OH

A

hydroxyl group (different than OH-)

32
Q

Which acid contains oxygen?

33
Q

Oxyacid naming

A

polyatomic ion -ous acid
“ “ - ic acid

34
Q

Binary naming

A

hydro- anion- ic acid

35
Q

Molar mass is the sum of the ___ ___ of each atom in the compound. Also known as molecular weight or molecular mass.

A

atomic masses

36
Q

Mass percent formula

A

= (mass part/mass whole)*100%

37
Q

Empirical formulas are formulas derived from __ ___ data.

A

mass percent

38
Q

Steps for finding the empirical formula

A
  1. determine the mass (g) of each element from mass%
  2. convert the mass of each element to moles and use the atomic mass of each element as the conversion factor
  3. divide all of the moles by the smallest number of moles
39
Q

Molecular formula is the ___ formula multiplied by an integer

40
Q

When a metal and nonmetal react, the ___ tends to lose electrons and the ___ tends to gain electrons.

A

metal, nonmetal

41
Q

Who discovered the during a chemical reaction the total mass of all compounds remains the same?

42
Q

Stoichiometry is based on what law?

A

Law of Conservation of Mass

43
Q

Percent error formula

A

[(theoretical-actual)/theoretical]*100%

44
Q

Molarity formula

A

(moles of solute)/ (liters of solution)

45
Q

Solute that increases the electrical conductivity of a solvent WHEN ADDED TO A SOLUTION is called a(n) ___.

A

electrolyte

46
Q

Solute that does NOT change the electrical conductivity when added to a solvent is a(n)

A

nonelectrolyte

47
Q

When a(n) ___ substance dissolves in water, it breaks up into its component Ions, which makes it a strong ___ regardless of how soluble it is.

A

ionic, electrolyte

48
Q

Substances that dissolve only to give molecules in a solution are/aren’t conductive and therefore are non/electrolytes

A

aren’t, nonelectrolytes

49
Q

All molecular substances dissolve as molecules, true or false?

50
Q

All ionic compounds are strong electrolytes, true or false?

A

True, because they will produce virtually nothing other than ions.

Freshman (semester 1) (10 decks)

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