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CHEM111 > Compounds and the Mole > Flashcards

Compounds and the Mole Flashcards

1
Q

Chemical nomenclature

A

the systemic approach to naming chemical compounds

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2
Q

Chemical formulas

A

combine elemental symbols and subscripts to represent compounds

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3
Q

Chemical formula of rust

A

Fe2O3

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4
Q

Molecular compounds

A

individual particles made up of bonded atoms known as molecules

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5
Q

Molecular compounds aka

A

covalent compounds

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6
Q

Covalent bonds are between

A

nonmetal atoms

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7
Q

Ionic compounds

A

extended 3D lattice structure (network) of atoms

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8
Q

Ionic compound composition

A

metal atoms + nonmetal atoms

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9
Q

Which 7 elements form diatomic molecules?

A

H2, N2, O2, F2, Cl2, Br2, I2

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10
Q

Allotropes

A

different molecular forms of an element

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11
Q

Carbon allotropes

A

diamond, graphite, nanotubes, fullerenes

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12
Q

mono-

A

1

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13
Q

di-

A

2

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14
Q

tri-

A

3

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15
Q

tetr(a)-

A

4

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16
Q

pent(a)-

A

5

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17
Q

hex(a)-

A

6

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18
Q

hept(a)-

A

7

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19
Q

oct(a)-

A

8

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20
Q

non(a)-

A

9

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21
Q

dec(a)-

A

10

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22
Q

N2O

A

dinitrogen monoxide

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23
Q

NH3

A

ammonia

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24
Q

PH3

A

phosphine

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25
Q

ArH3

A

arsine

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26
Q

metal atoms transfer electrons to

A

nonmetal atoms

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27
Q

Metal atoms tend to form

A

cations

28
Q

nonmental atoms tend to form

A

anions

29
Q

Polyatomic Ions

A

groups of two or more bonded atoms that have lost or gained electrons and thus have an overall net charge

30
Q

three types of cations

A

polyatomic, monatomic (constant charge), monatomic (variable charge)

31
Q

two types of anions

A

monatomic, polyatomic

32
Q

What is the only common polyatomic cation

A

ammonium ion, NH4+

33
Q

denote variable charge

A

roman numerals

34
Q

Oxyanions

A

contain one nonmetal atom plus a variable number of Oxygen atoms

35
Q

Common Oxyanions

A

Per __ate, __ate, __ite, hypo__ite

36
Q

ClO4-

A

Perchlorate

37
Q

ClO3-

A

chlorate

38
Q

ClO2-

A

chlorite

39
Q

ClO-

A

hypochlorite

40
Q

Per__ate

A

4 Oxygen atoms, except PO4^3-

41
Q

___ate

A

PO4^3-, as well as most with 3 Oxygen atoms, except SO3^2-

42
Q

__ite

A

SO3^2-, plus 2 Oxygen atoms

43
Q

Hypo__ite

A

One oxygen atom

44
Q

Hydrates

A

ionic compounds that contain water molecules

45
Q

anhydrous form

A

heated hydrate

46
Q

Acids

A

a special class of hydrogen-containing covalent compounds that, when dissolved in water, release one or more H+ ions and form an anion with a -1 charge for each H+ ion that was released

47
Q

Ionizable hydrogen atoms

A

the term for the H atoms that are released in water and are written at the beginning of the formula

48
Q

two types of acids

A

binary and oxyacids

49
Q

Binary acids

A

contain H atoms and atoms of an element from group 16 or 17; named as hydro-+root+-ic acid

50
Q

Oxyacids

A

hydrogen atoms bonded to oxyanions

51
Q

chemical counting unit

A

mole

52
Q

Avogadro’s Number

A

6.022 x 10^23 units/mol

53
Q

number of units calculation

A

number of moles x ((6.022 x 10^23 units)/1mol)

54
Q

How many moles of H2O are in a drop of water that contains 1.67 × 10^21H2O molecules?

A

1.67 x 10^21 H2O molecules x ((1 mol H2O)/(6.022 x 10^23 H2O molecules) = 2.77 x 10^-3 mol H2O

55
Q

How many moles of each element are in 1 mol of sucrose, C12H22O11?

A

12 mol C, 22 mol H, and 11 mol O

56
Q

Calculation for moles of atoms

A

moles of compound x chemical formula = moles of atoms

57
Q

Conversion of Molar Mass

A

moles of atoms x molar mass = mass of atoms

58
Q

Atomic Mass

A

the average mass of an atom, expressed in u

59
Q

Molecular Mass

A

the average mass of a molecule, expressed in u

60
Q

Formula mass

A

the average mass of a formula unit of any type of substance

61
Q

molar mass

A

the mass of any type of substance, using the same numerical value, but expressed in grams per mole

62
Q

Calculation of percent composition

A

(total mass of element in the compound)/(total mass of the compound) x 100%

63
Q

empirical formula

A

the simplest whole-number ratio of atoms in the compound

64
Q

Type of compound identified by empirical formula

A

ionic compound

65
Q

type of compound identified by a molecular formula

A

covalent

66
Q

molecular formula

A

the actual number of atoms of each element in one molecule of a covalent compound

67
Q

combustion analysis

A

a lab technique used to determine the empirical formula of compounds containing C, H, and possibly O

CHEM111 (5 decks)

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