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Fall 2017 > CHEM 105 Chapter 4 Quiz > Flashcards

CHEM 105 Chapter 4 Quiz Flashcards

1
Q

ionic bonding is between

A

a metal and a nonmetal

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2
Q

covalent bonding is between

A

nonmetals

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3
Q

ionic bonds involve

A

the transfer of electrons from one atom to the other (the metal atom becomes the cation (loses e-) and the nonmetal atom becomes the anion (gains e-))

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4
Q

the result of ionic bonding is

A

an ionic compound, which in the solid phase is composed of a lattice

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5
Q

covalent bonds involve

A

the sharing of electrons between two atoms

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6
Q

a compound is represented by its

A

chemical formula, the type and number of each element present in the compound

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7
Q

types of chemical formulas

A

empirical, molecular, structural

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8
Q

empirical formula

A

gives the relative number of atoms of each element in a compound; the simplest whole number (ratio) representation of the type and number of elements present in a molecule

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9
Q

molecular formula

A

gives the actual number of atoms of each element in a molecule of a compound

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10
Q

the molecular formula (can/cannot) be the same as an element’s empirical formula

A

can

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11
Q

structural formula

A

a sketch or diagram of how the atoms in the molecule are bonded to each other; it uses lines to represent covalent bonds

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12
Q

Lewis structure model

A

represents an element’s valence electrons as dots

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13
Q

Why does the Lewis structure focus on valence electrons?

A

chemical bonding involves the transfer or sharing of valence electrons between two or more atoms

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14
Q

“Octet Rule”

A

when atoms bond, they tend to gain, lose, or share e-s to result in a noble gas-like configuration

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15
Q

lattice energy

A

the extra stability that accompanies the formation of the crystal lattice; the energy released when the solid crystal forms form separate ions in the gas state; depends on size of charges and inversely on distance b/w ions

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16
Q

ionic compounds can be categorized into two types

A
  1. metal forms only one type of ion

2. metal forms more than one type of ion

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17
Q

naming binary ionic compounds of type I cations

A

[name of cation] + [base name of anion (+ -ide)]

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18
Q

naming type II binary ionic compounds

A

[name of cation] + (charge of cation in roman numerals) + [base name of anion (+ -ide)]

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19
Q

oxyanions

A

anions containing oxygen and another element

20
Q

naming oxyanions

A

according to the number of oxygen atoms in the ion

if there are two ions in the series, the one with MORE oxygen atoms has the ending -ate and the one with LESS oxygen atoms has the ending -ite

if there are more than two ions in the series, then the prefixed hypo- (less than) and per- (more than) are used (e.g. hypo-?-ite, ?-ite, ?-ate, per-?-ate)

21
Q

naming ionic compounds containing polyatomic ions

A

named in the same manner as binary ionic compounds, except the name of the polyatomic ion is used (e.g. NaNO2 is sodium nitrite)

22
Q

hydrated ionic compounds

A

hydrates are ionic compounds containing a specific number of water molecules associated with each formula unit (e.g. MgSO4 * 7 H2O is magnesium sulfate heptahydrate)

23
Q

common hydrate prefixes

A 
hemi 1/2
mono 1
di 2
tri 3
tetra 4
penta 5
hexa 6
hepta 7
octa 8
24
Q

covalent bonding: bonding pairs

A

electrons that are shared by atoms

25
Q

covalent bonding: lone pairs

A

electrons that are not shared by atoms but belong to a particular atom (AKA nonbonding pairs)

26
Q

single covalent bonds

A

when two atoms share one pair of electrons

27
Q

double covalent bond

A

when two atoms share two pairs of electrons

28
Q

triple covalent bond

A

when two atoms share three pairs of electrons

29
Q

the formula for a molecular compound (can/cannot) be readily determined from its constituent elements because ?

A

cannot; the same combination of elements may form different molecular compounds, each with a different formula (e.g. Nitrogen and Oxygen form NO, NO2, N2O, N2O3, etc.)

30
Q

molecular compounds

A

composed of two or more nonmetals

31
Q

naming molecular compounds

A
  1. write the name of the element with the smallest group number first (if the two elements lie in the same group, then write the element with the greatest row number first)
  2. the prefixes given to each element indicate the number of atoms present

[(prefix) + (name of 1st element)] + [(prefix) + (base name of 2nd element + -ide)]

32
Q

prefixes for molecular compounds (same as hydrates)

A 
mono 1 (usually omitted)
di 2
tri 3
tetra 4
penta 5
hexa 6
hepta 7
octa 8
nona 9
deca 10
33
Q

molecular mass

A

the mass of an individual molecule or formula unit; the mass of one mole of that compound

34
Q

determining a compound’s molecular mass

A

sum of the masses of the atoms in a single molecule or formula unit

35
Q

the percentage of each element in a compound can be determined from

A
  1. the formula of the compound
  2. the experimental mass analysis of the compound

% mass of element Z = [(molecular mass of element Z) / (mass of 1 mol of compound)] x 100%

36
Q

how to determine a chemical formula from experimental data

A

elemental analysis: masses of elements formed when a compound is decomposed, or that react together to form a compound (combustion analysis); percent composition

37
Q

finding an empirical formula

A
  1. convert the percentage to grams
  2. convert mass (g) to moles
  3. divide all by the smallest number of moles to obtain the atom-to-atom ratio for each of the elements in the compound
  4. multiply all mole ratios by a number to make all whole numbers
38
Q

to determine the molecular formula for a compound given the empirical formula,

A

molecular formula = (empirical formula) * n

n = (molar mass) / (empirical formula molar mass)

39
Q

combustion analysis

A

a common technique for analyzing compounds is to burn a known mass of compound and weight the amount of product made; by knowing the m ass of the product and composition of constituent element in the product, the original amount of constituent element can be determined

40
Q

early chemists divided compounds into two types

A

organic and inorganic

41
Q

organic compounds

A

compounds from living things; easily decomposed, cannot be made in lab

42
Q

inorganic compounds

A

compounds from the nonliving environment; very difficult to decompose but able to be synthesized

43
Q

organic compounds are mainly made of

A

C and H, sometimes with O, N, P, and S

44
Q

the main element that is the focus of organic chemistry is

A

carbon

45
Q

carbon bonding

A

carbon atoms bond almost exclusively covalently; when carbon bonds, it forms four covalent bonds; unique b/c can form limitless chains of C atoms, both straight and branched, and rings of C atoms

Fall 2017 (24 decks)

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