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Chem 151 > Week 3 (Naming) > Flashcards

Week 3 (Naming) Flashcards

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1
Q

prefix for 1

A

mono-

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2
Q

prefix for 2

A

di-

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3
Q

prefix for 3

A

tri-

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4
Q

prefix for 4

A

tetra-

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5
Q

prefix for 5

A

penta-

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6
Q

prefix for 6

A

hexa-

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7
Q

prefix for 7

A

hepta-

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8
Q

prefix for 8

A

octa-

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9
Q

prefix for 9

A

nona-

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10
Q

prefix for 10

A

deca-

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11
Q

Naming of Cations

A

-monoatomic cations bear same name as their elements (ex. Na+ = sodium ions, Ca(2+) = calcium ion)
-some metals can form more than one type of cation (ex. Cu+ = copper(I) ion, Cu(2+) = copper(II) ion)
-Polyatomic cations (NH4(+) = ammonium ion, H3O(+) = hydronium ion)

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12
Q

Naming of Anions

A

-simple anions end in -ide (Cl- = chloride ion, O(2-) = oxide ion, N(3-) = nitride ion)
-Polyatomic anions end in -ite or -ate (SO3(2-) = sulfite ion, ClO(-) = hypochlorite ion)

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13
Q

Inorganic Acids

A

compounds containing H+ and a simple anion (Binary acids, ex. HCl, H2S) or polyatomic anion (Oxo acids, ex. HNO3, H2SO4)

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14
Q

Naming Ionic Compounds

A

-name the cation, then name the anion (ex. CaCl2 = calcium chloride, NH4NO3 = ammonium nitrate)

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15
Q

Naming Covalent Compounds

A

-name the electropositive element, then name the electronegative element like an anion
-electronegative element ends in -ide
-use prefixes to indicate the number of each kind of atom in a molecule (CO2 = carbon dioxide, SO3 = sulfur trioxide)

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16
Q

Ammonia

A

NH3

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17
Q

Naming Inorganic acids

A

-names of acids are based on the names of the anions in the acids
-(-ide = hydro-…-ic acid) (ex. HCl = hydrochloric acid)
-(-ate = -ic acid) (ex. HNO3 = nitric acid)
-(-ite = -ous acid) (ex. HNO2 = nitrous acid)

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18
Q

Naming Inorganic compounds flowchart

A

-Does it carry charges? (If yes, name it as ion)
-Is it an acid (if yes, name the acid)
-Is it ionic or covalent?

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19
Q

Superoxide ion

A

O2(-)

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20
Q

Peroxide ion

A

O2(2-)

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21
Q

Hydrate

A

compounds in which water molecules (H2O) are bound to another element/compound
(ex. CuSO4 x 5H2O = Copper(II) sulfate pentahydrate)

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22
Q

Hygroscopic substances

A

absorb moisture from air to form hydrate, usually appear sticky or wet

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23
Q

Anhydride

A

a substance without water

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24
Q

Element order of Covalent Compound

A

1st: central element
2nd: peripheral element

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25
Q

Polyatomic ions (+1 charge)

A

-Hydronium (H3O+)
-Ammonium (NH4+)

26
Q

Polyatomic ions (-1 charge)

A

-Nitrate (NO3-)
-Nitrite (NO2-)
-Cyanide (CN-)
-Hydroxide (OH-)
-Perchlorate (ClO4-)
-Chlorate (ClO3-)
-Chlorite (ClO2-)
-Hypochlorite (ClO-)

27
Q

Polyatomic ions (-2 charge)

A

-Carbonate (CO3)
-Sulfate (SO4)
-Sulfite (SO3)

28
Q

Polyatomic ions (-3 charge)

A

Phosphate (PO4)

29
Q

Oxyanions

A

-family of polyatomic ions that have same central atom and varying numbers of oxygen
-prefix of per- indicates +1 oxygen than -ate ion (perchlorate and chlorate)
-prefix of hypo indicates -1 oxygen than -ite ion (hypochlorite and chlorite)

30
Q

Concentration

A

how much of the chemical solute is present in a solution

31
Q

Concentration unit

A

expresses the amount of solute chemical being dissolved per unit of solution/solvent (the most common unit is molarity)

32
Q

Solute

A

dissolved substance

33
Q

Solvent

A

liquid in which a solute is dissolved

34
Q

solution

A

mixture of solvent and solute

35
Q

Molarity (M)

A

amount of moles (n) in a solute per unit volume (L) of solution (n/L)

36
Q

Mole

A

scientific unit for measuring large quantities of very small entities such as atoms or molecules (6.022 x 10^23)

37
Q

Electronegativity

A

-a chemical property that describes the tendency of an atom or functional group to attract electrons toward itself
-increases from left to right across periods on periodic table, decreases down groups
-most electronegative is F, with rest of halogens + O also being highly electronegative
-metals have low (<2), nonmetals have high (>2)

38
Q

Semimetals

A

-have electronegativity around 2
-form ladder between metals and nonmetals on periodic table
-B, Si, Ge, As, Sb, Te, At

39
Q

Metallic behavior

A

-low electronegativity (electrons held loosely)
-malleable and shiny
-high melting points
-good conductors of electricity and heat

40
Q

Non-metallic behavior

A

-high electronegativity (electrons held tightly)
-brittle and dull
-wide range of melting points and boiling points
-poor conductor of electricity

41
Q

Electricity

A

conducted by mobile charged particles (electrons, ions, holes)

42
Q

Dissolving of substances

A

-ionic compounds dissociate to form cations and anions in water
-positive and negative charges of water are oppositely attracted to components in ionic compounds
-covalent compounds have little to no dissociation in water

43
Q

Major Species

A

the most abundant chemical entities present in a solution (ex. major species in NaCl solution are Na+ and Cl-) (ex. major species in CH2O solution is CH2O)

44
Q

Solubility Compounds

A

NAGSAG (nitrates, ammonium salts, group 1, sulfates, acetates, group VII)
-Salts containing group 1 metals
-Salts containing NH4+
-Salts containing NO3-, ClO3-, and CH3COO-
-Salts containing Cl-, Br-, and I- (except Pb(2+), H(2+), and Ag+)
-Compounds of SO4(2-) (except salts of Pb(2+), Hg(2+), and Ba(2+))

45
Q

H3O(+)

A

Hydronium

46
Q

NH4(+)

A

Ammonium

47
Q

NO3(-)

A

Nitrate

48
Q

NO2(-)

A

Nitrite

49
Q

CN(-)

A

Cyanide

50
Q

OH(-)

A

Hydroxide

51
Q

ClO4(-)

A

Perchlorate

52
Q

ClO3(-)

A

Chlorate

53
Q

ClO2(-)

A

Chlorite

54
Q

ClO(-)

A

Hypochlorite

55
Q

CO3(2-)

A

Carbonate

56
Q

SO4(2-)

A

Sulfate

57
Q

SO3(2-)

A

Sulfite

58
Q

PO4(3-)

A

Phosphate

59
Q

CH3COO(-)

A

acetate

60
Q

CH3COOH

A

acetic acid

61
Q
A

Chem 151 (7 decks)

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