Compounds and the Mole Flashcards
(67 cards)
1
Q
Chemical nomenclature
A
the systemic approach to naming chemical compounds
2
Q
Chemical formulas
A
combine elemental symbols and subscripts to represent compounds
3
Q
Chemical formula of rust
A
Fe2O3
4
Q
Molecular compounds
A
individual particles made up of bonded atoms known as molecules
5
Q
Molecular compounds aka
A
covalent compounds
6
Q
Covalent bonds are between
A
nonmetal atoms
7
Q
Ionic compounds
A
extended 3D lattice structure (network) of atoms
8
Q
Ionic compound composition
A
metal atoms + nonmetal atoms
9
Q
Which 7 elements form diatomic molecules?
A
H2, N2, O2, F2, Cl2, Br2, I2
10
Q
Allotropes
A
different molecular forms of an element
11
Q
Carbon allotropes
A
diamond, graphite, nanotubes, fullerenes
12
Q
mono-
A
1
13
Q
di-
A
2
14
Q
tri-
A
3
15
Q
tetr(a)-
A
4
16
Q
pent(a)-
A
5
17
Q
hex(a)-
A
6
18
Q
hept(a)-
A
7
19
Q
oct(a)-
A
8
20
Q
non(a)-
A
9
21
Q
dec(a)-
A
10
22
Q
N2O
A
dinitrogen monoxide
23
Q
NH3
A
ammonia
24
Q
PH3
A
phosphine
25
ArH3
arsine
26
metal atoms transfer electrons to
nonmetal atoms
27
Metal atoms tend to form
cations
28
nonmental atoms tend to form
anions
29
Polyatomic Ions
groups of two or more bonded atoms that have lost or gained electrons and thus have an overall net charge
30
three types of cations
polyatomic, monatomic (constant charge), monatomic (variable charge)
31
two types of anions
monatomic, polyatomic
32
What is the only common polyatomic cation
ammonium ion, NH4+
33
denote variable charge
roman numerals
34
Oxyanions
contain one nonmetal atom plus a variable number of Oxygen atoms
35
Common Oxyanions
Per __ate, __ate, __ite, hypo__ite
36
ClO4-
Perchlorate
37
ClO3-
chlorate
38
ClO2-
chlorite
39
ClO-
hypochlorite
40
Per__ate
4 Oxygen atoms, except PO4^3-
41
___ate
PO4^3-, as well as most with 3 Oxygen atoms, except SO3^2-
42
__ite
SO3^2-, plus 2 Oxygen atoms
43
Hypo__ite
One oxygen atom
44
Hydrates
ionic compounds that contain water molecules
45
anhydrous form
heated hydrate
46
Acids
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
Ionizable hydrogen atoms
the term for the H atoms that are released in water and are written at the beginning of the formula
48
two types of acids
binary and oxyacids
49
Binary acids
contain H atoms and atoms of an element from group 16 or 17; named as hydro-+root+-ic acid
50
Oxyacids
hydrogen atoms bonded to oxyanions
51
chemical counting unit
mole
52
Avogadro's Number
6.022 x 10^23 units/mol
53
number of units calculation
number of moles x ((6.022 x 10^23 units)/1mol)
54
How many moles of H2O are in a drop of water that contains 1.67 × 10^21 H2O molecules?
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
How many moles of each element are in 1 mol of sucrose, C12H22O11?
12 mol C, 22 mol H, and 11 mol O
56
Calculation for moles of atoms
moles of compound x chemical formula = moles of atoms
57
Conversion of Molar Mass
moles of atoms x molar mass = mass of atoms
58
Atomic Mass
the average mass of an atom, expressed in u
59
Molecular Mass
the average mass of a molecule, expressed in u
60
Formula mass
the average mass of a formula unit of any type of substance
61
molar mass
the mass of any type of substance, using the same numerical value, but expressed in grams per mole
62
Calculation of percent composition
(total mass of element in the compound)/(total mass of the compound) x 100%
63
empirical formula
the simplest whole-number ratio of atoms in the compound
64
Type of compound identified by empirical formula
ionic compound
65
type of compound identified by a molecular formula
covalent
66
molecular formula
the actual number of atoms of each element in one molecule of a covalent compound
67
combustion analysis
a lab technique used to determine the empirical formula of compounds containing C, H, and possibly O
