Quiz 4 - Chemical Bonds and Nomenclature of Compounds

Lattice energy

_________________ is used to measure the stability of an ionic compound and relative strength of an ionic bond

True

True or False:

The more negative the lattice energy, the stronger the ionic bond and the more stable the ionic compound

(Q1 x Q2)/d

What equation is used to solve for lattice energy?

- Charges of ions

- distance between ions

Lattice energy = (Q1 x Q2)/d

- Q1 and Q2 are the ________________

- d is the ________________________

NaF

- Na+ and F- are closer together than Na+ and Cl-

- d of NaF is smaller, making E_e1 greater

Which has a stronger ionic bond?

NaCl vs. NaF

True

True or False:

Magnitude in charge usually has a greater impact in relative ionic strength

MgCl2

- larger magnitude in charge, leading to greater attraction between ions

What has a stronger ionic bond?

NaCl vs. MgCl2

1 - 1+

2 - 2+

13 - 3+

14 - 4-

15 - 3-

16 - 2-

17 - 1-

What is the charge for

1. Group 1

2. Group 2

3. Group 13

4. Group 14

5. Group 15

6. Group 16

7. Group 17

Mg^2+ Br^- →

MgBr_2

Write the ionic compound formula between Mg and Br

Fe^2+ Cl^-

FeCl_2

or

Fe^3+ Cl^-

FeCl_3

Write the ionic compound formula between Fe and Cl

Al^3+ O^2-

2(Al^3+) → 6+ 3(O^2-) → 6-

6+ and 6- cancel out

→ Al2O3

Write the ionic compound formula between Al and O

more than one

Parentheses indicate that there is _______________ Polyatomic ion in a compound

Iron (III) chloride

Identify the nomenclature:

FeCl3

Transitional

______________ metals form more than one cation

Roman Numerals

_______________ in nomenclature are used to indicate charge for transitional metals

Mono → 1

Di → 2

Tri → 3

Tetra → 4

Penta → 5

Hexa → 6

Hepta → 7

Octa → 8

Nona → 9

Deca → 10

If there is a hydrate, prefixes are used to indicate how many water molecules are present.

list all 10 hydrate prefixes:

Iron (III) chloride hexahydrate

Identify the nomenclature:

FeCl3 6H2O (hydrate)

They all consist of 2 atoms making them diatomic Molecules

What do these molecules have in common?

H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂

Phosphorus trichloride

Identify the nomenclature:

PCl3

anion

Binary acids in aqueous solution derive their name from the __________________

polyatomic ions

Oxoacids in aqueous solution derive their name from ____________________

add

starting hydro-

ending -ic.

To identify the nomenclature for Binary acids in aqueous solution, you __________________

Hydrochloric acid

Binary acids: Identify the nomenclature:

HCl (aq)

add ending-ic from ending -ate

add ending -ous from ending -ite

To identify the nomenclature for Oxoacids in aqueous solution, __________________

hypo-

per-

Oxoacids in aqueous solutions:

Anions that have a __________ or ___________ prefix keep the prefix in the name

Nitric acid (from nitrate)

Oxoacids: Identify the nomenclature:

NHO3 (aq)

Nitrous acid (from nitrite)

Oxoacids: Identify the nomenclature:

NHO2 (aq)

Perchloric acid

Oxoacids: Identify the nomenclature:

HClO4 (aq)

1. Mn^2+ Br^- → MnBr2

2. Ba^2+ NO_3 ^- → Ba(NO3)2

3. K^+ OH^- → KOH

Identify formulas:

1. Manganese (II) bromide

2. Barium nitrate

3. Potassium hydroxide

1. Iron (II) perchlorate

2. Barium chloride

3. Strontium nitrate

Identify the nomenclature:

1. Fe (ClO4)2

2. BaCl2

3. Sr(NO3)2

1. diphosphorus pentachloride

2. nitrogen trifluoride

3. dinitrogen monoxide

4. S3 O5

Identify nomenclature/formulas:

1. P2 Cl5

2. NF3

3. N2O

4. Trisulfur pentoxide

Oxacids (polyatomic ion)

- Hypochlorous acid

Binary acids (anion)

- Hydroiodic acid

Identify the nomenclature:

1. HClO (aq)

2. HI (aq)

1. Nitric acid (oxoacid)

2. Nitrate (polyatomic ion)

Identify the nomenclature:

1. NHO3

2. NO3