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Chemistry 1a > Ch 3 - Molecules, Compounds, and Chemical Equations > Flashcards

Ch 3 - Molecules, Compounds, and Chemical Equations Flashcards

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1
Q

Chemical Bonds

A

Compounds are made of atoms held together by these(Ionic and Covalent)

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2
Q

(Ionic Compounds)Naming Monatomic Nonmetal Anion

A

add “ide” to the end of the anion name.

Nitride, Oxide, Sulfide…

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3
Q

(ionic Compounds)Naming Metals with invariant charge

A

the cation name is the metal name as it has no variation in what it can be.

Lithium, Sodium, Potassium…

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4
Q

(Ionic Compounds)Naming Metals with variant charge

A

Used when a meta(the cation)l has more than one ion.

Chromium, Cr^2+, Chromium (II), Chromous

Chromium Cr^3+. Chromium (III), Chromic

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5
Q

Ionic Bond

A

Results when electrons have been transferred between atoms creating Ions.

Usually a metal(cation) and a nonmetal(anion)

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6
Q

Covalent Bond

A

Results when two atoms share some of their electrons.

Usually between nonmetals

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7
Q

Molecular Compound

A

Composed of molecules and almost always contain ONLY nonmetals

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8
Q

Ionic Compound

A

Almost always contain a metal with a nonmetal.

Use Empirical formula with ionic compounds

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9
Q

Chemical Formula

A

indicates the elements present in the compound and the relative number of atoms or ions of each.

H2O gives the atoms composing it and the ratio.

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10
Q

Empirical Formula

A

Gives the lowest whole number ratio of atoms of each element in a compound.

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11
Q

Molecular Formula

A

Gives the exact number of atoms of each element in a compound.

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12
Q

Structural Formula

A

Use with Covalent bonds to show connections.

H2O2 H-O-O-H

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13
Q

Ball and Stick Model

A

molecular model with balls and stick to show atoms

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14
Q

Space Filling Molecular Model

A

Orbs connected to each other to represent how an atom would look

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15
Q

Molecular Compound

A

two or more covalently bonded nonmetals

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16
Q

Ionic Compound

A

composed of cations(metals) and anions(nonmetals)

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17
Q

Formula Unit

A

In an Ionic Compound, the smallest electrically neutral collection of ions.

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18
Q

Polyatomic Ion

A

an ion composed of two or more atoms.

19
Q

Binary Compound

A

compound with only two different elements.

20
Q

Naming Binary Compound

A

Name of cation(metal), basename of anion(nonmetal) + ide.

KCl, Potassium Chloride

21
Q

Naming Binary Ionic Compounds with more than 1 charge

A

name of cation(metal), charge of cation in roman numberl, base of anion + ide

CuO, Copper(II) Oxide

It is Copper(II) because Oxygen is O^2- and the charge must balance to be neutral

22
Q

Oxyanions

A

anions containing oxygen and another element

Many polyatomic ions are this.

23
Q

(Polyatomic ions)Hypo, ite, ate, per

A

Used if an element has more than two ion variations(the anion).

ClO^- Hypochlorite
ClO2^- Chlorite
ClO3^- Chlorate
ClO4^- Perchlorate

24
Q

Hydrate(Ionic Compounds)

A

used to state a specific amount of water molecules associated with a formula unit.

BaCl2* 6H2O Barium Chloride Hexahydrate

25
Q

Naming Binary Molecular Compounds

A

Prefix,name of 2st element, prefix, base name of second element + ide

BF3, Boron Triflouride

26
Q

Mono

A

1

27
Q

Di

A

2

28
Q

Tri

A

3

29
Q

Tetra

A

4

30
Q

Penta

A

5

31
Q

Hexa

A

6

32
Q

Hepta

A

7

33
Q

Octa

A

8

34
Q

Nona

A

9

35
Q

Deca

A

10

36
Q

Acid

A

molecular compounds that release hydrogen ions(H^+) when dissolved in water.

Sour taste, ability to dissolve metals

37
Q

Naming Binary Acids

A

composed of H^+ and a nonmetal

Hydro, base name of nonmetal + ic, acid

HCl(aq), Hydrochloric Acid

38
Q

Naming Oxyacids

A

contain H^+ and an oxyanion.

Oxyanion ending with “-ate”
SO4^2-, Sulfate -> Sulfuric Acid

Oxyanion ending with “-ite”
H2SO3(aq) Sulfite -> Sulfurous Acid

39
Q

Formula mass

A

the sum of the atomic masses of all the atoms in its chemical formula.

CO2 -> 12.01amu+2(16.00amu) = 44.01amu

40
Q

Molar Mass

A

the mass in grams of 1 mol of a substance or formula units.

CO2 -> 44.01amu, 44.01, formula mass, and 44.01 molar mass

41
Q

Mass Percent Composition(Mass Percent)

A

an elements % of the compounds totals

CCl2F2

mass % Cl = ((2)(molar mass Cl)/Molar mass CCl2F2) * 100

42
Q

Elemental Analysis

A

Used to take data and turn it into a chemical formula.

base sample out of 100g, use %s as subscripts for components, divide each by their molar mass, divide by the lowest number of a component to get whole numbers(Empirical Formula)

43
Q

Determine Molecular Formula from Empirical Formula

A

Empirical formula = CH
Molecular Weight = 78.1134g/mol

fivide by CH weight(13.02g/mol)

78.1134/13.02 = 6

C6H6

Chemistry 1a (15 decks)

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