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Chem 112 > Chem Ch 3 > Flashcards

Chem Ch 3 Flashcards

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1
Q

Chemical bonds

A

Formed because of the attractions between charged particles. Ionic or covalent.

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2
Q

Ionic bonds

A

Between metals and nonmetals. Involved the transfer of electrons from one atom (metal) to another (nonmetal).

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3
Q

Covalent bonds

A

Between 2 or more nonmetals. Involve sharing of electrons between two atoms. Shared electrons have a lower potential energy than they would in the isolated atoms because they interact with the nuclei of both atoms.

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4
Q

Ionic compound

A

Result of ionic bond. Is composed of a lattice of alternating cations and anions in solid phase.

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5
Q

Lattice

A

A regular 3-dimensional array

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6
Q

Molecular compound

A

Covalently bonded compund. Each molecule is an independent entity (not covalently bound to other molecules. Nonmetal with nonmetal.

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7
Q

Chemical formula

A

Indicates which elements are present in the compound and the relative number of atoms or ions of each. H2O. Lists most metallic first.

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8
Q

3 types of chemical formulas

A

Empirical, molecular, structural

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9
Q

Empirical formula

A

Relative number of atoms of each element in a compound. HO.

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10
Q

Molecular formula

A

Actual number of atoms of each element in a compound. H2O2. Always a whole number multiple of the empirical formula.

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11
Q

Structural formula.

A

Uses lines to represent covalent bonds.
H2O2: H-O-O-H
CO2: O=C=O

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12
Q

Molecular model

A

More accurate and complete way to specify a compound. Ball and stick or space filling.

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13
Q

Atomic elements

A

Exist in nature with single atoms as their base units. Most elements.

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14
Q

Molecular elements

A

Exist as molecules. Most are diatomic, few polyatomic.

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15
Q

Diatomic elements

A

Oxygen, Hydrogen, Nitrogen, Fluorine, Chlorine, Bromine, Iodide.

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16
Q

Polyatomic elements

A

Phosphorous, Sulfur, Selenium.

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17
Q

Basic unit of molecular compounds

A

Molecules composed of constituent atoms

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18
Q

Basic unit of ionic compounds

A

Formula unit - smallest electrically neutral collection of ions (ie: NaCl in sodium chloride. 1:1 ratio. No single Na pairs with Cl)

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19
Q

Polyatomic ion

A

Has a charge. Covalently bonded atoms. Found in ionic compounds.

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20
Q

Oxyanions

A

Anions containing oxygen and another element.

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21
Q

Hydrates

A

Ionic compounds with specific numbers of water molecules associated with each formula unit. Given a numerical prefix.

22
Q

Why can’t formulas for molecular compounds be easily determined based on its constituent elements?

A

The same group of elements may form many different molecular compounds, each with a different formula.

23
Q

Acids

A

Molecular compounds that release hydrogen ions (H+) when dissolved in water. Composed of hydrogen and one or more nonmetals (written second). HCl is a molecular compound that forms H+ and Cl- ions when dissolved in water. Always aqueous. HCl (g) would be hydrogen monochloride instead of Chloric acid.

24
Q

Binary acids and naming them

A

Composed of hydrogen and a nonmetal. (Hydro) + (element + ic) + (acid). Hydrobromic acid, HBr.

25
Q

Oxyacids and naming them

A

Oxyacids contain hydrogen and an oxyanion (anion containing a nonmetal and oxygen). Ending with ate, (base name of oxyanion + ic) + (acid). Ending in ite, (base name of oxyanion + ous) + (acid). HNO3: Nitric acid. H2SO3: Sulfurous acid.

26
Q

Formula mass

A

Average mass of a compound. (# of 1st element * atomic mass of 1st element) + (# of 2nd element * atomic mass of 2nd element)

27
Q

Acetate

A

C2H3O2, CH3OOH

28
Q

Carbonate

A

CO3, charge 2-. If H in front, bicarbonate or hydrogen carbonate.

29
Q

Hydroxide

A

OH-

30
Q

Nitrite

A

NO2-

31
Q

Nitrate

A

NO3-

32
Q

Chromate

A

CrO4, charge 2-

33
Q

Phosphate

A

PO4, charge 3-

34
Q

Ammonium

A

NH4+

35
Q

Hypochlorite

A

ClO-

36
Q

Chlorite

A

ClO2-

37
Q

Chlorate

A

ClO3-

38
Q

Perchlorate

A

ClO4-

39
Q

Permanganate

A

MnO4-

40
Q

Sulfite

A

SO3, charge 2-

41
Q

Hydrogen sulfite or bisulfite

A

HSO3, charge 2-

42
Q

Sulfate

A

SO4, charge 2-

43
Q

Cyanide

A

CN-

44
Q

Peroxide

A

O2, charge 2-

45
Q

Molar mass of a compound

A

Mass in grams of 1 mol of its molecules or formula units. Numerically equivalent to its formula mass. g/mol.

46
Q

Mass percent composition

A

An elements percentage of the compound’s total mass. mass percent = (molar mass of element X in 1 mol of compound/molar mass of the compound) x 100

47
Q

Combustion analysis

A

A way to obtain empirical formulas for unknown compounds. The unknown compound undergoes burning in the presence of pure oxygen. Carbon converts to CO2, hydrogen converts to H2O.

48
Q

Chemical reaction

A

A process in which one or more substances are converted into one or more different substances.

49
Q

Combustion reaction

A

Type of chemical reaction in which a substance combines with oxygen to form one or more oxygen containing compounds. Emit heat = provide energy.

50
Q

Reactants and products

A

Substances on left, substances on right

Chem 112 (3 decks)

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