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CHEM-1315 > Unit 4.3: Explain bonding in ionic compounds including trends in lattice energy > Flashcards

Unit 4.3: Explain bonding in ionic compounds including trends in lattice energy Flashcards

1
Q

Reading 6.1: Ionic Bonding

In an ionic bond, the _ atom transfers electrons to the _ atom.

A

metal
nonmetal

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2
Q

Reading 6.1: Ionic Bonding

What holds ionic bonds together?

A

The ions attract each other due to opposite charges created by the transfer of electrons.

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3
Q

Reading 6.1: Ionic Bonding

The forces of attraction between oppositely charged species

A

Electrostatic Attraction

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4
Q

Reading 6.1: Ionic Bonding

Identify the ions that are created in a bond between calcium and bromine.

A

Ca2+
B-

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5
Q

Reading 10.10: Latice Energy

The energy released when gas-phase ions combine to form a solid ionic compound.

A

Lattice Energy

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6
Q

Reading 10.10: Latice Energy

The energy needed to break a mole of a specific type of bond

A

Bond Energy

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7
Q

Reading 10.10: Latice Energy

The direct transition from solid phase to gas phase.

A

Sublimation

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8
Q

Reading 10.10: Latice Energy

Write the chemical equation that corresponds to the lattice energy of CaCl2

A

Ca2+(g) + 2 Cl-(g) = CaCl2(s)

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9
Q

Reading 10.10: Latice Energy

Write the chemical equation that corresponds to the lattice energy of stronium nitride, Sr3N2

A

3 Sr2+(g) + 2 N3-(g) = Sr3N2(g)

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10
Q

Reading 10.10: Latice Energy

Bond length in ionic compounds (decreases/increases) as atomic radii increases

A

Increases

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11
Q

Reading 10.10: Latice Energy

The lattice energy of an ionic compound (increases/decreases) in magnitgude (becomes less exothermic) as the size of one or more of the ions increases.

A

Decreases

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12
Q

Reading 10.10: Latice Energy

Lattice energy tends to be more (negative/positive) when it increases in magnitude.

A

Negative

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13
Q

Reading 10.10: Latice Energy

Lattice energies tend to be (smaller/larger) in magnitude for ionic compounds consisting of ions with large charges.

A

Larger

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14
Q

Reading 10.10: Latice Energy

Arrange the lattice energies in order from least negative to most negative:
MgCl2
NaF
CsF
ScN

A

CsF
NaF
MgCl2
ScN

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15
Q

Reading 10.10: Latice Energy

Arrange the lattice energies of the following compounds in order from least negative to most negative:
MgO
NaCl
CaO
Al2O3

A

NaCl
CaO
MgO
Al2O3

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16
Q

4.3 Lecture Notes

Extremely

A

releases heat

17
Q

4.3 Lecture Notes

What is the array assembled in an ionic compound called?

A

Crystalline lattice

18
Q

4.3 Lecture Notes

In ionic solids, ions _ and _ in all directions

A

attract
repel

19
Q

4.3 Lecture Notes

The distance between ions in an ionic bond

A

Bond Length

20
Q

4.3 Lecture Notes

Which two factors influence lattice energy?

A
  1. Ion size
  2. ion charge
21
Q

4.3 Lecture Notes

When disrupted, the crystal lattice is (stable/unstable)

A

Unstable

22
Q

4.3 Lecture Notes

Ionic compounds have (high/low) melting and boiling points.

A

High

23
Q

4.3 Lecture Notes

All ionic compounds are (solids/liquids/gasses) at room temperature

A

Solids

24
Q

4.3 Lecture Notes

Breaking down the srystalline solid requires a (lot of/little) energy

A

A lot

25
Q

4.3 Lecture Notes

The stronger the attraction, the (smaller/larger) the lattice energy.

A

Larger

26
Q

4.3 Lecture Notes

The stronger the attraction (the larger the lattice energy), the (higher/lower) the melting point.

A

Higher

27
Q

4.3 Lecture Notes

The melting point of ionic compounds is generally greater than what temperature?

A

> 300 degrees celcius

28
Q

4.3 Lecture Notes

What is requried for a material to conduct electricity?

A

It must have charged particles that are able to flow through the material.

29
Q

4.3 Lecture Notes

What state do ionic compounds conduct electricity in and why?

A

Molten and aqueous because the ions can move.

30
Q

4.3 Lecture Notes

Endothermic

A

requires heat

31
Q

4.3 Lecture Notes

What three things does the attraction between opposite charges do in ionic compounds?

A
  1. Draws ions together
  2. Releases energy
  3. Causes ions to assemble into a crystalline lattice
32
Q

4.3 Lecture Notes

The formation of a crystal lattice is (endothermic/exothermic)

A

Exothermic

33
Q

4.3 Lecture Notes

Why is lattice energy reported with a negative sign?

A

The system lost energy

34
Q

4.3 Lecture Notes

What three things does lattice energy depend upon?

A
  1. Ion Size
  2. Ion Charge
  3. Arrangment of the ions in the solid
35
Q

4.3 Lecture Notes

Longer bonds = (smaller/larger) lattice energy

A

Smaller

36
Q

4.3 Lecture Notes

Less attractive force = (smaller/larger) lattice energy

A

Smaller

37
Q

4.3 Lecture Notes

The larger the charges, the (smaller/larger) the lattice energy

A

Larger

CHEM-1315 (27 decks)

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