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Chemistry 110 > (Ch.5) Molecules & Compounds > Flashcards

(Ch.5) Molecules & Compounds Flashcards

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1
Q

Describe the Law of Constant Composition.

A

Compounds display constant composition. This means any sample of a compound will have the same ratio of atoms within it.
(ex. H20= 8.0 grams of O:1.0 gram of H)

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2
Q

What will be left if a compound decomposes?

A

Their original elements will remain.

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3
Q

What is a Chemical Formula?

A

A chemical formula represents the number and type of atoms in a compound.
(ex. H20, 2 hydrogen, 1 oxygen)

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4
Q

How do we decide what atom is listed first when writing compounds? There are two rules.

A
  1. Metals are listed first.
  2. The more metallic element is listed first.
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5
Q

How do you determine which element is “more metallic?”

A

The element further to the bottom. (vertically)
The element further to the left. (horizontally)

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6
Q

Describe a Empirical Formula.

A

This formula shows the simplest whole number ratio of atoms in a compound.
(ex. HO instead of H2O2, just a simplified ratio)

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6
Q

What are the two primary types of Chemical Formulas?

A
  1. Empirical Formulas
  2. Molecular Formulas
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6
Q

What is a Polyatomic Ion?

A

These are groups of atoms that act as a unit and have a charge. (Ion with more than one atom)

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7
Q

Describe a Molecular Formula.

A

This formula shows the actual number of atoms of each element in a compound.
(ex. H2O2 instead of HO)
(This is a kind of Chemical Formula)

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8
Q

What are the four primary models/formulas used to represent a molecule?

A
  1. The Molecular Formula
  2. The Structural Formula
  3. The Ball & Stick Model
  4. The Space-Filling Model.
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9
Q

Describe the Structural Formula.

A

This model shows each atoms ARE connected to one another, along with how many of each they are.
H
H-C-H
H

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10
Q

Describe the Ball and Stick Model.

A

This model helps us visualize the molecules SHAPE. The atoms are balls and the bonds are sticks.

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11
Q

Describe the Space-Filling Model.

A

This is our best representation of how atoms actually look. Making molecules look like a bunch of large circles stuffed together.

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12
Q

Elements have two subcategories. What are they?

A
  1. Atomic Elements
  2. Molecular Elements
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13
Q

Compounds have two subcategories. What are they?

A
  1. Ionic Compounds
  2. Molecular Compounds
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14
Q

What is a Molecular Compound? What is their base unit?

A
  1. These are compounds composed of 2 or more NON-metals.
  2. Molecules
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15
Q

What is an Ionic Compound? What is their base unit?

A
  1. These are compounds composed of a metal and a non-metal.
  2. Formula Unit
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16
Q

How do you differentiate between an Atomic and Molecular Element?

A

Atomic Elements have singular atoms as their base unit.
Molecular Elements are Diatomic- meaning they always naturally appear in pairs as their base unit.

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17
Q

What is a Diatomic Molecule?

A

This is the base unit of a Molecular Element.

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18
Q

There are seven naturally occurring Diatomic Molecules. What are they?

A

BO(o) FINCH
-Bromine
-Oxygen
-Fluorine
-Iodine
-Nitrogen
-Chlorine
-Hydrogen

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19
Q

Describe electron transfer and charges in a ionic compound.

A
  1. Metals typically loose electrons, non-metals typically suck up electrons.
    SO…the metal gives up it’s electron(s) to the non metal.
  2. Metal (+) cation
    Non-metal (-) anion
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20
Q

How do you write a chemical formula for ionic compounds?
Ex. What is the formula of the ionic compound formed from Al(3+) and N(3-)?

A
  1. You switch the charges of each ions and place them as the other’s subscript.
  2. Al(3)N(3)~ AlN
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21
Q

What are the two types of Ionic Compounds?

A
  1. Type I Binary
  2. Type II Binary
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22
Q

What is a Type I Binary Ionic Compound?

A

This is where the charge on the cation (metal atom/s) does not vary.

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23
Q

What is a Type II Binary Ionic Compound?

A

The charge on the cation (metal) does vary.

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24
Q

What is a polyatomic atom?

A

a bonded group of atoms with a charge

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25
Q

Differentiate between a Type I Binary/ Type II Binary Ionic Compound.

A

T1: The cation doesn’t vary.
T2: The cation varies.

26
Q

What is the formula for naming a Type I Binary Ionic Compound?
Ex. MgO, CaO, AlS

A
  1. (name of the cation + base name of the anion + ide)
  2. magnesium oxide, calcium oxide, aluminum sulfide

ps. The cation is the name of the more metallic element. Then it’s the the base name of the non-metallic element.

27
Q

What is the naming formula for a Type II Binary Ionic Compound? (without any polyatomic ions)
Ex. CuCl2, FeN2, HgCl

A
  1. (name of the cation+ charge of the cation + base name of the anion+ide.)
  2. Copper II Chloride, Iron II Nitride, Magnesium II Chloride
28
Q

What are the primary five ions with variable charge? List their chemical symbols as well.

A
  1. (Fe) Iron
  2. (Cu) Copper
  3. (Sn) Tin
  4. (Pb) Lead
  5. (Hg) Mercury
29
Q

What is an Oxyanion?

A

A negatively charged ion that contains oxygen.

30
Q

What is the naming pattern of an ionic compound w/polyatomic atoms?

ex. Al2(SO4)3

A

(name of the cation + Type I or II + name of anion/polyatomic atom+ ite/ate)

ex. Aluminum Sulfate

31
Q

Name the polyatomic ions and their charges.
NO3
NO2

A
  1. Nitrate (-)
    (higher charge=”ate”)
  2. Nitrite (-)
    (lower charge=”ite”)
32
Q

Name the polyatomic ions and their charges.
PO4
H2PO4
HPO4

A
  1. Phosphate (-3) ♥️
  2. Dihydrogen Phosphate (-)
  3. Hydrogen Phosphate (-2)
33
Q

Name the polyatomic ions and their charges.
SO4
HSO4
SO3

A
  1. Sulfate (-2)
  2. Hydrogen Sulfate (-)
  3. Sulfite (-2)
    ♥️ Is there a pattern to their charges?
34
Q

Name the polyatomic ions and their charges.
CO3
HCO3

A
  1. Carbonate (2-)
  2. Hydrogen Carbonate (-)
35
Q

Name the polyatomic ions and their charges.
CIO
CIO2
CIO3
CIO4

A
  1. Hypochlorite (-)
  2. Chlorite (-)
  3. Chlorate (-)
  4. Perchlorate (-)
    ♥️ Why do these all have the same charge if there are different number of oxygen atoms?
36
Q

Name the polyatomic ions and their charges.
NH4
OH
CN
C2H3O2

A
  1. Ammonium Ion (+) ♥️
  2. Hydroxide (-)
  3. Cyanide (-)
  4. Acetate (-)
37
Q

What is the typical naming pattern for polyatomic atoms?

A

Hypo_____ite
___________ite
___________ate
Per_______ate

38
Q

What is the naming pattern of ions with variable charge?

A

The ion with a higher charge ends with “ic”.
The ion with the lower charge ends with “ous.”

39
Q

Fe (Iron) has variable charges. What are it’s two variations?

A
  1. Fe II (+2) Ferrous
  2. Fe III (+3) Ferric
    (positive charge cuz it’s a metal)
40
Q

Cu (Copper) has variable charges. What are it’s two variations?

A
  1. Cu I (+) Cuprous
  2. Cu II (2+) Cupric
41
Q

Sn (Tin) has variable charges. What are it’s two variations?

A
  1. Tin II (2+) Stannous
  2. Tin IV (+4) Stannic
42
Q

Pb (Lead) has variable charges. What are it’s two variations?

A
  1. Pb II (2+) Plumbous
  2. Pb IV (4+) Plumbic
43
Q

Hg (Mercury) has variable charges. What are it’s two variations?

A
  1. Hg2 I (2+) Mercurous
  2. Hg II (2+) Mercuric
44
Q

What would you name a molecular compound?

A

A Type III Binary Compound.♥️

45
Q

What is the naming pattern of a molecular compound?

A

(prefix + name of the first element + prefix + base name of the second element + ide)
the prefix tells you the number of atoms!

46
Q

What is the purpose of the prefix in molecular compounds?

A

It lets you know the number of atoms in each element.

47
Q

What are the prefixe for 1-10?

A
  1. Mono
  2. Di
  3. Tri
  4. Tetra
  5. Penta
  6. Hexa
  7. Hepta
  8. Octa
  9. Nona
  10. Deca
48
Q

These are molecular compounds… how would you say them?
1. N2O3
2. P7S8
4. BCl4

A
  1. Dinitrogen trioxide
  2. Heptaphosphorus octasulfide
  3. Boron tetrachloride
49
Q

What is an acid?

A

A molecular compound that produces H+ ions in water.

50
Q

What are the two types of acids?

A
  1. Binary Acids
  2. Oxyacids
51
Q

When we are given an acid what is our first step?

A

Determine if the acid is a Binary or Oxy acid.

52
Q

What is a Binary Acid? Give an example.

A
  1. An acid that includes hydrogen and another non-metal.
  2. (ex. HCl=hydrochloric acid)
53
Q

What is an Oxyacid?

A

An acid that includes oxygen, hydrogen, and a non-metal.

54
Q

What is the naming convention for Binary Acids?
ex. HF
HI
HBr

A
  1. (hydro + base name of the non-metal + “ic” + acid)
  2. (ex. Hydrofluoric acid)
    (ex. Hydroiodic acid)
    (ex. Hydrobromic acid)
55
Q

What are the two exceptions for Binary Acids that he gave us?

A
  1. HCN- hydrocyanic acid (because CN is cyanide)
  2. H2S- hydrosulfuric acid (rather than hydrosulfic acid, cuz that would make too much sense)
56
Q

What is the naming pattern for an Oxyacid? Give an example.

A
  1. If the name of the oxyanion ends in “ite” (base name of oxyanion + “ous” + acid)
    If the name of the oxyanion ends in “ate”
    (base name of oxyanion+ “ic” + acid)
  2. ## HNO2, the oxyanion is NO2. This is called nitrous acid.HNO3, the oxyanion is NO3. This is called nitric acid.
57
Q

What are the two exceptions for Oxyacids?

A
  1. H3PO3- phosphorus acid
    H3PO4- phosphoric acid
  2. H2SO3- sulfurous acid
    H2SO4- sulfuric acid
    (They both just flow better this way I suppose?) ♥️
58
Q

What is a Hydrate?

A

Any compound that contains water.

59
Q

What does it mean to be Hygroscopic?

A

This means a compound absorbs water from it’s surroundings.

60
Q

What does a hydrate look like? What is the naming pattern for a hydrate?

A
  1. BaCl2 (2H2O)- Barium Chloride Dihydrate
  2. (name of the compound + # of water molecules + hydrate)
61
Q

What is the common name for a diatomic molecule?

A

A molecular element.

62
Q

Write a formula for the compound that forms between Sr and Br.

A

SrBr2- Bromine is written as Br2 as it is a diatomic molecule/molecular compound.

63
Q

What is the formula for chlorite?

A

ClO2

64
Q

Name the compound CrCl3.

A
  1. This is an ionic compound.
  2. Cr, Chromium has various charges
  3. What is the charge of Cl3? (Cl=-1, Cl3=-3) So, Cr has a charge of 3+, thus being Cr (III); add the ide cuz it’s a compound.
    ANSWER: Chromium (III) Chloride

Chemistry 110 (13 decks)

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