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Principles of Chemistry 1 > U3 - Module 3: Characterizing Ionic Networks > Flashcards

U3 - Module 3: Characterizing Ionic Networks Flashcards

1
Q

What are the common physical characteristics of ionic compounds?

A
  • Rigid
  • Crystalline
  • Mainly solid
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2
Q

What role does covalent bonds play in a molecular compound?

A

Connects the molecules within the compound together.

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3
Q

What type of interactions are intermolecular forces considered?

A

Electrostatic interactions

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4
Q

Electrostatic Interactions

A

Interactions between electron rich and electron poor regions

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5
Q

What two things need to be identified when analyzing an ionic compound?

A
  • Physical size
  • Charges of each molecular section
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6
Q

Explain the difference between CH3Cl and NaCl that cause them to have different physical characteristics.

A

CH3Cl: Composed of nonmetals held together by covalent bonding, which has them share their valence electrons.

NaCl: Two charged particles (ions) that are held together by ionic bonding (charged based)

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7
Q

Ionic Compounds

A

Result from the combination of metal and nonmetal atoms.

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8
Q

What factor plays a big role in the different charges of ionic compounds.

A

The EN differences.
- Metals are more positive while nonmetals are more negative.

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9
Q

What does a larger EN difference between bonding atoms indicate?

A

A more polar bond

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10
Q

What is the EN rule for ionic compounds?

A

The EN difference between the metal and nonmetal needs to be greater than 2.0 to be considered ionic.

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11
Q

Where do the bonding atoms spend most of their time in an ionic compound?

A

Near the nonmetal atom because it is more negative, and the bonding atoms have the valence electrons that are attracted to the nonmetal.

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12
Q

How do you use the ionization energy diagrams to determine what ions will likely form between 2 atoms?

A
  1. Use the peaks to determine the electron configurations for each atom.
  2. Compare the number of valence electrons between the two, and identify if there are any unfilled subshells.
  3. If an atom has unfilled subshells, try to complete the subshells by moving the valence electrons between the two.
  4. The atom that loses valence electrons become more positive and the atom that gains becomes more negative.
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13
Q

When are atoms most stable?

A

When they have completely filled valence electron orbitals.
- Noble gases

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14
Q

What role does the metal play in an ionic compound?

A

The positive ion; cation

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15
Q

What role does the nonmetal play in an ionic compound?

A

The negative ion; anion

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16
Q

What happens when metal and nonmetal atoms interact?

A

They create ions
-Positive and negative charged particles

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17
Q

What is the temperature effect on ion ordering?

A

High Temp: Disrupts the order of ions due to them gaining energy and vibrating more intensely.

Low Temp: The ions create an ordered formation due to the low energy environment, causing less motion.

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18
Q

What happens to the ion ordering when the volume decreases?

A

As volume decreases, the ions have less space to move around, and create a formation of a solid.
- Anions want to be surrounded by cations, and cations want to be surrounded by anions (1:1 ratio).

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19
Q

Ionic Networks

A

Positive and negative ions interact with other ions in the system but do not form molecules.

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20
Q

How do ions in an ionic network arrange?

A

Into a crystalline ionically bonded network.

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21
Q

What is the only thing the chemical formula indicates in an ionic network?

A

The ratio of + to - ions in the grid (1:1)

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22
Q

Why do metals have a positive charge and nonmetals have a negative charge?

A

Metals commonly lose valence electrons to become stable while nonmetals gain valence electrons to become stable.

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23
Q

What is the charge of Al as a cation?

A

+3

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24
Q

What is the charge of C as an anion?

A

-4

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25
What is the main goal of atoms losing/gaining electrons?
To obtain a noble gas configuration - Most stable
26
What is the net charge of an ionic network that forms?
No net charge
27
What does a net charge of 0 mean in an ionic network?
The anions and cations combine in ratio that adds to 0 (neutral).
28
Why are ionic compounds packed closely together?
To minimize energy
29
Charge Neutrality
The amount of anions is the same as the amount of cations = 0
30
Compare size changes for anions and cation.
Anions: Have a large radius due to having more electrons in the electron cloud. Cations: Have smaller radius due to having less electrons in the electron cloud.
31
What is unique about the ionic charges of transition metals?
They have multiple charges - Has to be stated in the formula name with roman numerals
32
How do ionic compounds exist?
As networks of ions in rigid structures that maximize electrostatic attraction with overall charge neutrality.
33
How do you name ionic compounds with one possible charge?
1. Have the metal name (no change) 2. Have the nonmetal name - Add ide to the end
34
What is the charge of Zn?
+2
35
What is the charge of Ag?
+1
36
What is the charge of Cd?
+2
37
What are the charges of groups 1 and 2 of metals?
Group 1: +1 Group 2: +2
38
How do you name ionic compounds where the metal has multiple possible charges?
1. Write the metal name - Add the roman numeral in paranthesis of the charge after the metal name. 2. Write the nonmetal name - Add ide to the end
39
Hydrates
Compounds where the ionic compounds contain a portion of water molecules.
40
What is the chemical formula of hydrates called?
Water of hydration
41
How do you write the ionic compound names for hydrates?
1. Write the ionic name of the compound. - With or without roman numerals depending on the metal ion. 2. Write hydrate, but add the prefix for the amount of water molecules present before.
42
How do you identify when an ionic compound is a hydrate?
Water is present within the chemical formula.
43
Name CaCl2
Calcium Chloride
44
Name FeF3
Iron (III) Fluoride
45
Name BaCl2 * 2H2O
Barium Chloride Dihydrate
46
What is the formula for Sodium Bromide?
NaBr
47
What is the formula for Lead (IV) Sulfide?
PbS2
48
What is the formula for NiF2 * 4H2O
Nitrogen Fluoride Tetrahydrate
49
What is the difference between ionic compounds that end in -ate vs - ite.
Compounds that end in "ate" have one more oxygen then their similar compounds that end in "ite"
50
How do you name a polyatomic ion that is combined with a nonmetal?
1. State the polyatomic ion name 2. State the nonmetal name - Add ide
51
Name NH4 Cl
Ammonium Chloride
52
How do you name a polyatomic ion that is combined with another polyatomic ion?
1. State the polyatomic cation name (+) 2. State the polyatomic anion name (-)
53
Name (NH4)2 SO4
Ammonium Sulfate
54
How do you name a polyatomic ion that is combined with a metal?
1. State the metal name - Include parenthesis if needed 2. State the polyatomic anion name
55
Write the chemical formula for a reaction between Ca and O2.
CaO
56
Write the chemical formula for a reaction between Ca and N2.
Ca3 N2
57
How do you determine what the best submicroscopic representation is for an ionic solid?
1. Determine the ion ratio between the anion and cation. - Number of molecules in representation should equal the ratio. 2. Have the ions packed closely together. - Ionic solids for the crystalline networks, where the ions are as close as they possibly can be.
58
What do different ionic compounds have?
Different crystal structures
59
What is the difference between "Face centered cubic" and "Body centered cubic"?
FCC- Each face has one atom in the middle, with other atoms around the corners. BCC- There is one atom in the center of the entire cube, with atoms on each corner of the center atom (makes a cube).
60
What are the two types of crystal structures?
Face centered cubic (FCC) and Body centered cubic (BCC)
61
Describe the different physical characteristics of FCC and BCC crystal structures.
FCC- Softer, high density and ductile (bendable) = When ions are tightly structured, force t their structure will cause the ions to bend, rather that completely dissociate. BCC- Harder, less density, and more brittle (breakable) = The atoms are less tightly packed because their are less atoms around the center. The structure lacks enough molecules to have them slide over each other when a force is added, so instead of bending they break.
62
Unit Cell
Smallest repeating units that create a crystal lattice
63
Crystal Lattice
The repeating 3D arrangements of molecules/atoms/ions in a crystalline solid.
64
What are the two properties of ionic solids?
1. Ionic compounds do not conduct electricity as solids, but do when they are melted into liquids. 2. Solid ionic compounds shatter when they are struck with a force (brittle).
65
Describe the difference between electron movement in ionic solids and metals.
Ionic Solids- Electrons are localized around the atom and do not move (Cl- does not lose the - charge) Metals- Electrons can freely move between atoms.
66
What does the movement of electrons explain about the conductivity of electricity.
Molecules that can conduct electricity can have the electrons freely move around the molecule.
67
Why do ionic compounds conduct electricity only as a liquid?
The electrons of an ionic compound as a liquid can freely move around due to the intermolecular forces being decreased as energy is applied.
68
Why do ionic compounds shatter easily when struck with a force as a solid?
Since the ions are packed so closely, the force moves similar forces near each other, causing them to repel and the substance to break.
69
Ionic Bonds
An INTRAmolecular force that results in bonds between ions.
70
What is the strongest type of molecular force?
Ionic Bonds
71
What do ionic compounds tend to be?
Solids with high melting/boiling points
72
What two variables are needed to determine the properties of ionic compounds?
1. Charge of ions 2. Size of compound
73
Coulomb's Law
Energy = (charge of cation)*(charge of anion) ÷ radius^2
74
What is the general size patterns of anions and cations?
Anions - Larger molecules due to adding electrons Cations - Smaller molecules due to removing electrons
75
How do you determine the general radius of ionic compounds?
Base the radius off of the atomic size pattern of the periodic table (smaller for gases, larger for solids)
76
What determines the properties of an ionic compound?
electrostatic forces among ions, between ions, and between surrounding particles
77
What two factors strengthens the force of an ionic compound?
1. Larger charges 2. Smaller the radius
78
What two factors weaken the force of an ionic compound?
1. Smaller charges 2. Larger the radius
79
How does the force strength of ionic compounds relate to the melting point?
The stronger the force of an ionic compound, the higher the melting point of the compound.
80
How do you differentiate between molecular and ionic compounds?
Molecular Compound - Nonmetals bonded together Ionic Compound - Ions bonded together - Nonmetals and metals
81
What is the rule for determining if an ionic compound is soluble?
If you multiply the two charges together... q * q < 4 = soluble q * q ≥ 4 = insoluble
82
How can polyatomic ions form ionic compounds?
The charge of an can combine with an ion that has an opposing charge, creating an ionic compound.
83
Explain why NaCl absorbs energy when dissolved in water.
Na+ and Cl- ions adopt a larger number of configurations with water when they are mixed with each other.
84

Principles of Chemistry 1 (14 decks)

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