S.2.1

Question 1

What is the ionic model?

Answer 1

A model that explains ionic bonding through the attraction between oppositely charged ions.

Question 2

What is lattice enthalpy?

Answer 2

A measure of the strength of the ionic bond in a crystal lattice.

Question 3

What is the relationship between ionic charge and lattice enthalpy?

Answer 3

Ionic charge = ionic attraction = lattice enthalpy.

Question 4

How does ionic radius affect lattice enthalpy?

Answer 4

A larger ionic radius results in lower attraction of ions and lower lattice enthalpy.

Question 5

Which ions have greater lattice enthalpy?

Answer 5

Ions with larger charge density due to their smaller radius.

Question 6

What are the physical properties of ionic compounds?

Answer 6

High melting points, high boiling points, and low volatility.

Question 7

True or False: Ionic compounds can dissolve in polar liquids.

Answer 7

True.

Question 8

Fill in the blank: The tendency of a substance to vaporize is known as _______.

Answer 8

volatility.

Question 9

What suffix is used to finish the names of ions?

Answer 9

-ide.

Question 10

What must be true about the charges of cations and anions in a salt?

Answer 10

The charges of cation and anion should cancel each other out.

Question 11

What is the effective nuclear charge experienced by outer electrons?

Answer 11

Less than the full nuclear charge due to the shielding effect.

Question 12

What is the shielding effect?

Answer 12

Inner electrons reduce the attraction between the positively charged nucleus and outermost electrons.

Question 13

How does the number of protons relate to the number of electrons in an atom?

Answer 13

Atoms are electrically neutral; the number of protons equals the number of electrons.

Question 14

What occurs when oppositely charged ions meet?

Answer 14

They are pulled together by electrostatic attraction.

Question 15

What is a polyatomic ion?

Answer 15

A molecule with a charge.

Question 16

Define effective charge.

Answer 16

The net positive charge experienced by an electron, which is less than the full nuclear charge.

Question 17

What is the ionization energy trend between metals and non-metals?

Answer 17

Metals form +ions and have low ionization energies; non-metals form -ions and have high ionization energies.

Question 18

What does the ionic model assume about the structure of crystals?

Answer 18

That crystals are made up of spherical ions.

Question 19

What is the significance of the effective nuclear charge in ionic compounds?

Answer 19

It influences the size of ions and their ability to form bonds.

Question 20

What is the formula to calculate lattice enthalpy?

Answer 20

ΔHlattice | = k Q1Q2/ro

Question 21

What is the typical charge of sodium in ionic compounds?

Answer 21

+1.

Question 22

What is the typical charge of chlorine in ionic compounds?

Answer 22

-1.

Question 23

What type of reactions occur between elements that are furthest apart in the periodic table?

Answer 23

More vigorous reactions occur between elements that are furthest apart in the periodic table.

Question 24

What leads to greater ionic attraction?

Answer 24

Greater ionic charge leads to greater ionic attraction.

Question 25

What are ionization energies?

Answer 25

Ionization energies are the energy required to remove an atom.

Question 26

What happens to successive ionization energy after the first?

Answer 26

Successive ionization energy needed to remove every electron after the first increases.

Question 27

Why do ionization energies increase?

Answer 27

Energies increase because removing an atom makes it more positively charged, so the remaining electrons are held more tightly by the nucleus.

Question 28

What causes large jumps within ionization energies?

Answer 28

Large jumps occur because electrons are removed from more stable inner energy levels.

Question 29

What is the maximum oxidation state?

Answer 29

The maximum oxidation state is the number of electrons an atom can reasonably lose.

Question 30

What does oxidation state represent?

Answer 30

Oxidation state is the number that represents how many electrons the atom has gained, lost, or shared.

Question 31

When do you need to add Roman numerals to element names?

Answer 31

You need to add Roman numerals when an element has more than one common oxidation state.

Question 32

What is the characteristic of ionic compounds?

Answer 32

Ionic compounds are electrically neutral.

Question 33

What are polyatomic ions?

Answer 33

Polyatomic ions are made up of more than one atom which together have gained or lost an electron.

Question 34

What is the formula for nitrate?

Answer 34

The formula for nitrate is NO3-.

Question 35

What is the formula for sulfate?

Answer 35

The formula for sulfate is SO4^2-.

Question 36

What is the formula for phosphate?

Answer 36

The formula for phosphate is PO4^3-.

Question 37

What is the formula for hydroxide?

Answer 37

The formula for hydroxide is OH-.

Question 38

What is the formula for hydrogen carbonate?

Answer 38

The formula for hydrogen carbonate is HCO3-.

Question 39

What is the formula for carbonate?

Answer 39

The formula for carbonate is CO3^2-.

Question 40

What is the formula for ammonium?

Answer 40

The formula for ammonium is NH4+.

Question 41

What are some examples of acids?

Answer 41

Examples of acids include HNO3 (aq), H2SO4 (aq), H3PO4 (aq), H2O (l), H2CO3 (aq), HCl (aq).

Question 42

What type of bonding occurs within polyatomic ions?

Answer 42

Bonding within the polyatomic ion is covalent.

Question 43

What structure do ionic compounds have?

Answer 43

Ionic compounds have a lattice structure.

Question 44

What do formulas of ionic compounds represent?

Answer 44

Formulas are ratios of ions present.

Question 45

What are physical properties?

Answer 45

Physical properties are those that can be observed without chemically altering the substance.

Question 46

What is lattice enthalpy?

Answer 46

Lattice enthalpy is used as a measure of the strength of the ionic bond.

Question 47

What does a positive enthalpy change indicate?

Answer 47

A positive enthalpy change indicates that energy is needed to separate the ions.

Question 48

What factors affect lattice enthalpy?

Answer 48

Factors affecting lattice enthalpy include ionic charges and ionic radii.

Question 49

How do ionic charges affect lattice enthalpy?

Answer 49

Higher ionic charges lead to higher lattice enthalpy.

Question 50

How do ionic radii affect lattice enthalpy?

Answer 50

Larger ionic radii lead to lower lattice enthalpy.

Question 51

What happens when ions separate from a lattice?

Answer 51

As ions separate from a lattice, they become surrounded by water molecules.

Question 52

In what type of liquids are ionic compounds soluble?

Answer 52

Ionic compounds are soluble in polar liquids.

Question 53

What is the conductivity of ionic compounds in liquid and gaseous states?

Answer 53

Ionic compounds have high conductivity in the liquid and gaseous states.

Question 54

What happens to ionic compounds when force is applied?

Answer 54

When force is applied, ions of the same charge positioned next to each other cause repulsion, leading to the lattice splitting.

Question 55

What is a stereoisomer?

Answer 55

Compounds made of the same elements but with different spatial arrangements.