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CHEM1045 > Chapter 3 - Molecules, Compounds, And Chemical Equations > Flashcards

Chapter 3 - Molecules, Compounds, And Chemical Equations Flashcards

1
Q

The properties of a compound are ____ from the constituent elements.

A

Totally different (think H20 vs 0)

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2
Q

____ ____ are forces of attraction between atoms.

A

Chemical bonds

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3
Q

The bonding attraction comes from attraction between ____ and ____.

A

Protons and Electrons

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4
Q

___ bonds result when electrons have been transferred between atoms.

A

Ionic

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5
Q

When do Ionic bonds generally occur?

A

When metal atoms bond to nonmetal atoms.

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6
Q

____ bonds result when two atoms share some of their electrons.

A

Covalent

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7
Q

When do covalent bonds generally occur?

A

When nonmetal atoms bond together.

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8
Q

The number of ____ is written to the right of the element as a subscript.

A

Atoms

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9
Q
  • Gives the relative number of atoms of each element in a compound.
  • Does not describe how many atoms, the order of attachment, or shape.
  • Used for ionic compounds
A

Empirical Formula

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10
Q
  • Gives the actual number of atoms of each element in a molecule of a compound.
  • Does not describe the order of attachment, or the shape.
A

Molecular Formula

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11
Q
  • Uses lines to represent covalent bonds and shows how atoms in a molecule are connected or bonded to each other.
  • does not directly describe the 3D shape.
A

Structural Formula

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12
Q

Uses balls to represent the atoms and sticks to represent the attachments between them.

A

Ball-and-stick Models

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13
Q

Uses interconnected spheres to show the electron clouds of atoms connecting together.

A

Space-filling Models

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14
Q

Elements whose particles are single atoms

A

Atomic Elements

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15
Q

Elements whose particles are multi-atom molecules

A

Molecular Elements

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16
Q

Compounds whose particles are molecules made of only nonmetals

A

Molecular Compounds

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17
Q

Compounds whose particles are cations and anions

A

Ionic Compounds

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18
Q

____ elements occur as 2 atom molecules.

A

Diatomic

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19
Q

What is the rule of 7?

A
  • Remember Hydrogen
  • Go to Nitrogen (7)
  • Move 2 to the side and then 3 down
  • this creates a 7
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20
Q

Classify each of the following as either an atomic element, molecular element, molecular compound, or ionic compound

1) Aluminum, Al
2) Aluminium Chloride, AlCl3
3) Chlorine, Cl2
4) Acetone, C3H6O
5) Carbon Monoxide, CO
6) Cobalt, Co

A

1) Atomic Element
2) Ionic compound
3) Molecular Element
4) Molecular Compound
5) Molecular Compound
6) Atomic Element

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21
Q

Because we must balance the charge, if Na+ is combined with S2-, you will need ____ Na+ ions for every ____ S2-, therefore the formula must be ___

A

2 Na+ for every 1 S2-, resulting in Na2S

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22
Q

What is the Formula steps for Ionic Compounds?

A

1) Write the Symbol for the Metal cation and it’s charge
2) Write the Symbol for the nonmetal anion and it’s charge
3) Charge (without sign) becomes subscript for the other ion
4) Reduce subscripts to smallest whole number ratio
5) Check that the sum of the charges of the cations cancels the sum of the anions

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23
Q

What are the formulas for compounds made of the following ions?

1) Potassium ion with a nitride ion
2) Calcium ion with a bromide ion
3) Aluminum ion with a sulfide ion

A

1) K3N
2) CaBr2
3) Al2S3

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24
Q

To name a cation:

1) Metal with invariant charge =
2) Metal with variable charge=
3) Polyatomic ion =

A

1) Metal name
2) Metal name (charge)
3) Memorize

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25
Q

To name an anion:

1) Nonmetal =
2) Polyatomic ion =

A

1) Stem of nonmetal name + ide

2) Memorize

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26
Q

Naming Binary Ionic Compounds for Metals with Invariant Charge

A

1) Name Metal cation first, Name nonmetal anion
2) cation name is the metal name
3) nonmetal name is changed by adding -ide
Ex: CsF = Cesium Fluoride

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27
Q

Name the following compounds:

1) KCl
2) MgBr2
3) Al2S3

A

1) Potassium Chloride
2) Magnesium Bromide
3) Aluminum Sulfide

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28
Q

Naming Binary Ionic Compounds for Metals with variable charge

A

1) Name Metal cation first, Name nonmetal anion second
2) Metal cation name is the metal name followed by a Roman number in parentheses to indicate the charge
3) Nonmetal anion named by changing the ending on the nonmetal name to -ide

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29
Q

Name the following compounds:

1) TiCL4
2) PbBr2
3) Fe2S3

A

1) Titanium(IV) Chloride
2) Lead(II) Bromide
3) Iron(III) Sulfide

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30
Q

What are the formulas for compounds made from the following ions?

1) Copper(II) Ion with a Nitride Ion
2) Iron(II) Ion with a Bromide Ion

A

1) Cu3N2

2) FeBr2

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31
Q

____ are ionic compounds containing a specific number of waters for each formula unit.

A

Hydrates

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32
Q

In a formula, attached waters follow ___.

A

•, Ex: CoCl2•6H20

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33
Q

In name attached waters indicated by ____ + hydrate after name of ionic compound.

A

Prefix, Ex: Cobalt(II) Chloride Hexahydrate

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34
Q

Hydrate Prefixes

1) hemi
2) mono
3) di
4) tri
5) tetra
6) penta
7) hexa
8) hepta
9) octa

A

1) 1/2
2) 1
3) 2
4) 3
5) 4
6) 5
7) 6
8) 7
9) 8

35
Q

Writing Names of Binary Molecules Compounds of Two Nonmetals

A

1) Write Name of first element in formula
a) element furthest left and down
b) use the full name of the element
2) Writes Name the second element in the formula with an -ide suffix
3) Use prefix in front of each name to indicate the number of atoms
a) Never use the prefix mono- on the first element

36
Q

Name the following binary molecules:

1) BF3
2) NO2
3) PCl5
4) I2F7

A

1) Boron Trifluoride
2) Nitrogen Dioxide
3) Phosphorus Pentachloride
4) Diiodine Heptafluoride

37
Q

Write Formulas for the Following:

1) Dinitrogen Tetroxide
2) Sulfur Hexafluoride
3) Diarsenic Trisulfide

A

1) N204
2) SF6
3) As2S3

38
Q

What are some qualities of Acids?

A
  • Molecular compounds that form H+ when dissolved in water
  • Sour taste
  • Dissolve many metals (not noble metals)
  • Formula generally starts with H, Ex: HCl
39
Q

____ Acids habe H+1 cation and nonmetal anion (only two elements).

A

Binary

40
Q

____ have H+ cation and polyatomic anion.

A

Oxyacids

41
Q

Naming Binary Acids

A
  • Write a hydro prefix
  • Follow with the nonmetal name
  • Change ending on nonmetal name to -ic
  • Write the wird acid at the end of the name
42
Q

Name the binary acid HCl(aq)

A

Hydrochloric Acid

43
Q

Naming Oxyacids

A
  • If polyatomic ion Name ends in -ate, then change ending to -ic suffix
  • If polyatomic ion Name ends in -ite, then change ending to -ous suffix
  • Write wird acid at the end of all names
44
Q

Name the oxyacid H2SO4(aq)

A

Sulfuric Acid

45
Q

What are the formulas for the following acids?

1) Chlorous acid
2) Phosphoric Acid
3) Hydrobromic Acid

A

1) HClO2
2) H3PO4
3) HBr

46
Q

How many moles are in 50.0g of PbO2? (Pb = 207.2, O = 16.00)

A

0.209molPbO2

47
Q

What is the Mass of 4.78x1024 NO2 molecules?

A

365gNO2

48
Q

What can the percentage composition be determined by?

A
  • The formula of the compound

* The experimental mass analysis of the compound

49
Q

Formula for Percent Composition

A

Percentage = (part/whole) x 100%

50
Q

Find the mass percent of Cl in C2Cl4F2

A

69.58%

51
Q

The ____ ____ tells you the mass of a constituent element in 100g of compound.

A

Mass percent

52
Q

Benzaldehyde is 79.2% carbon. What mass of benzaldehyde contains 19.8g of C?

A

25.0g benzaldehyde

53
Q

Which formula is the simplest, whole-number ratio of the atoms of elements in a compound?

A

Empirical Formula

54
Q

Finding an Empirical Formula

A
  • Convert the percentages to grams (100g)
  • Convert grams to moles
  • Write a pseudo formula using moles as subscripts
  • Divide all by smallest number of moles
  • Multiply all mole ratios by number to make all whole numbers
55
Q

Determine the Empirical Formula of Stannous fluoride,which contains 75.7% Sn (118.70) and the rest fluorine (19.00)

A

Sn1F2

56
Q

Determine the Empirical Formula of magnetite, which contains 72.4% Fe (55.85) and the rest oxygen (16.00)

A

Fe3O4

57
Q

What do you need to determine the molecular formula?

A

You need to know the Empirical also formula and the molar mass of the compound.

58
Q

Benzopyrene has a molar mass of 252 g/mol and an empirical formula of C5H3. What is its molecular formula? (C =12.01, H= 1.01)

A

(252 g/mol/63.08 g/mol) = 4

59
Q
  • A common technique for analyzing compounds is to burn a known mass of compound and weight the amounts of product made.
  • Generally used for organic compounds containing C, H, O.
A

Combustion Analysis

60
Q
  • Involve chemical changes in matter resulting in new substances
  • Involve rearrangement and exchange of atoms to produce new molecules
A

Chemical Reactions

61
Q

• Shorthand way of describing a reaction
• Provides information about
- Formulas of reactants and products
- States of reactants and products
- Relative numbers of reactants and product molecules that are required
- Can be used to determine weights of reactants used and products that can be made

A

Chemical Equations

62
Q

Methane gas burns to produce ___ ___ gas and ____ ____.

A

Dioxide gas and gaseous water

63
Q

Whenever something burns it combines with

A

O2(g)

64
Q

To show the reaction obeys the Law of Conservation of Mass the equation must be

A

Balanced

65
Q

The (g) after the Formulas tells us the ____ of the chemical

A

State

66
Q

The number in front of each substance tells us the numbers of those molecules in a reaction

A

Coefficients

67
Q

An equation is balanced if

A

There are equal numbers of atoms of each element on the reactant and product sides

68
Q

Symbols indicating the state after chemicals

1) (g)
2) (l)
3) (s)
4) (aq)

A

1) gas
2) liquid
3) solid
4) aqueous = dissolved in water

69
Q

Energy symbols used above the arrow for decomposition reactions

1) D
2) hn
3) shock
4) elec

A

1) heat
2) light
3) mechanical
4) elec

70
Q

Write a balanced equation for Al(s) + O2(g) = Al2O3(s)

A

4Al(s)+3O2(g)= 2Al2O3(s)

71
Q

Write a balanced equation for

Al(s) + 6HC2H3O2(aq) = Al(C2H3O2)3(aq) + 3H2(g)

A

2Al(s) + 6HC2H302(aq) = 2Al(C2H302)3(aq) + 3H2(g)

72
Q

In the 18th Century, compounds from living things were called

A

Organic

73
Q

In the 18th Century, compounds from the nonliving environment were called

A

Inorganic

74
Q

____ compounds easily decomposed and could not be made in the 18th Century lab

A

Organic

75
Q

____ compounds were very difficult to decompose, but were able to be synthesized

A

Inorganic

76
Q

Today we commonly make ___ compounds in the lab and find them all around us.

A

Organic

77
Q

Organic compounds are mainly made out of

A

Carbon and Hydrogen, sometimes with O, N, S, P

78
Q

Carbon atoms bond almost exclusively

A

Covalently

79
Q

When Carbons bonds, it forms ____ covalent bonds

A

4

80
Q

Carbon is unique in that it can form ___ chains of C atoms, both straight and branched, and rings of C atoms.

A

Limitless

81
Q

What are the 2 main categories of organic compounds?

A

Hydrocarbons and functionalities hydrocarbons

82
Q

___ contain only C and H

A

Hydrocarbons

83
Q

Most files are mixtures of

A

Hydrocarbons

84
Q

What are some common hydrocarbons?

A

Methane, Propane, n-Butane, n-Pentane, Ethene, and Ethyne

CHEM1045 (7 decks)

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