Chapter 7 Outline

Ionic and Metallic Bonding

  • Section 7.1 – Ions
  • are the electrons in the ______occupied energy level.
  • are the only electrons involved in ______.
  • Elements in the same have the same ______of valence electrons.
  • are diagrams that show the of the element surrounded by the valence electrons are .
  • Practice Problems
  • Write the electron dot structure for the following elements:

P ArMgHe

  • The states that atoms tend to achieve a configuration when they have valence electrons.
  • tend to electrons to achieve noble-gas configuration. tend to ______electrons to achieve noble-gas configuration.
  • A ion is a ion that has ______electrons.
  • When writing the for a cation, write the electron configuration for the ______and then subtract the electrons from the ______energy level.
  • When you name a , the name of the ______does not change. Ex: Ca+2 =
  • Sample Problem
  • Write the electron configuration and name for the following:

Sr2+

Fe+3

  • Practice Problems
  • Write the electron configurations and the name for the following:

Zn+2

Na+

  • are charged ions that have ______electrons.
  • When writing the for anions, write the electron configuration for the and then the correct number of electrons.
  • When naming an , you change the ending of the element to . Ex: Cl- =
  • Sample Problems
  • Write the electron configuration and name for the following:

P-3

F-

  • Practice Problems
  • Write the electron configuration and name for the following:

Br-

S-2

  • Section 7.1 Assessment
  1. How can you determine the number of valence electrons in an atom of a representative element?
  1. Atoms of which elements tend to gain electrons? Atoms of which elements tend to lose electrons?
  1. How do cations form?
  1. How do anions form?
  1. How many valence electrons are in each atom?
  1. Potassium
  2. Carbon
  3. Magnesium
  4. Oxygen
  1. Draw the electron dot structure for each element in question 5.
  1. How many electrons will each element gain or lose in forming an ion?

a. calcium

b. fluorine

c. aluminum

d. oxygen

  1. Write the name and symbol of the ion formed when

a. a potassium atom loses one electron.

b. a zinc atom gains one electron

c. a fluorine atom gains one electron

  1. Write the electron configuration of Cd+2.
  • Section 7.2 – Ionic Bonds and Ionic Compounds
  • Compounds composed of are called .
  • Although they are composed of , ionic compounds are electrically .
  • The that hold ions together are called .
  • A shows the kinds and ______of atoms in the smallest representative unit of a substance.
  • A is the lowest ______

______of ions in an ionic compound.

  • When you charges to write the ______for an ionic compound, you must make the charge and charge equal by adding subscripts.
  • The must be in the ratio to be correct.
  • Sample Problems
  • Write the formula for the compound formed between the following elements.

Potassium and oxygen

Magnesium and nitrogen

  • Practice Problems
  • Write the formula for the compound when the following elements combine.

Potassium and iodine

Aluminum and oxygen

Calcium and chlorine

Barium and sulfur

  • are a group of atoms with an overall .
  • When charges for polyatomic ions, you follow the same of cancelling the + and – charge.
  • However, if you need to add a to a polyatomic ion, then you have to put the polyatomic ion in . Ex: Ca(NO3)2
  • Sample Problems
  • Write the formula for the compound when the following ions combine:

Sodium and phosphate

Ammonium nitride

Aluminum carbonate

  • Practice Problems
  • Write the formula for the compound when the following ions combine:

Barium nitrate

Lithium phosphate

Strontium sulfite

  • Properties of ionic compounds include the following:
  • solids
  • High points
  • Conduct when molten or aqueous
  • Made of ______
  • Made of ______
  • Made of ______
  • A is a substance with a repeating arrangement of particles called the .
  • The of an ion is the number ions of charge that surround the in a crystal.
  • Section 7.2 Assessment
  1. How can you describe the electrical charge of an ionic compound?
  1. What properties characterize ionic compounds?
  1. Write the correct chemical formula for the compounds formed by each pair of ions.

K+, S-2

Ca+2, O-2

Na+, O-2

Al+3, N-3

  1. Write formulas for each compound.

barium chloride

Magnesium oxide

Lithium oxide

Calcium fluoride

  1. Which pairs of elements are likely to form ionic compounds?

Cl, Br

Li, Cl

K, He

I, Na

  • Section 7.3 – Bonding in Metals
  • The of metal atoms can be modeled as a .
  • consist of the attraction of the free-floating valence for the positively charged .
  • are good conductors and ______because of their electrons.
  • are the most crystals because they contain type of element.
  • An is a mixture with ______properties.
  • A is made when atoms of one metal atoms of another metal.
  • An is made when ______metal atoms are inserted in larger metal atoms.
  • Section 7.3 Assessment
  1. How do chemists model the valence electrons in metal atoms?
  1. How can you describe the arrangement of atoms in metals?
  1. Why are alloys more useful than pure metals?
  1. Describe what is meant by ductile and malleable.
  • Section 9.1 – Naming with Regular Metals
  • A is a single atom with a charge. Ex:
  • When naming a , the name of the element does not . Ex: K+ =
  • When naming an , the ending of the element changes to . Ex: O-2 =
  • A ______is a group of atoms with an overall charge. Ex: SO4-2
  • Most polyatomic ions end in or . The ending does not change when naming a compound (unless it is an which we will talk about later).
  • The suffix indicates that the polyatomic ion contains one more than the polyatomic ion with the suffix. (Ex: sulfate = SO4-2, sulfite = SO3-2)
  • The are located in groups 1 and 2 (except for ). is also a regular metal.
  • When naming a compound that starts with a ______

______, you name the (cation) and add ____ to the nonmetal (anion). Ex: NaCl =

  • If the anion is a , then you do not change the . Ex: CaCO3 =
  • Sample Problems
  • Name the following compounds:

Na2O

AlBr3

Li2SO4

  • Practice Problems
  • Name the following compounds:

LiNO3

Ca2(PO4)3

(NH4)2O

  • When writing the of a compound that starts with a regular metal, you must ______

______.

  • Ex: aluminum bromide
  • Sample Problems
  • Write the formula for the following compounds:

Aluminum chloride

Calcium acetate

Lithium fluoride

  • Practice Problems
  • Write the formula for the following compounds:

Calcium carbonate

Aluminum oxide

Cesium oxalate

  • Section 9.1 Assessment
  1. What are the usual ending for the names of polyatomic ions?
  1. How does a polyatomic ion differ from a monatomic ion?
  1. Write the formula for these binary compounds.

Beryllium chloride

Cesium sulfide

Sodium iodide

Strontium oxide

  1. Write the formula for these compounds.
  1. sodium perchlorate
  1. magnesium hydrogen carbonate
  1. calcium acetate
  1. Identify any incorrect formulas. Explain your answer.
  1. Mg2(SO4)3
  1. Rb3As
  1. BeCl3
  1. NaF
  • Section 9.2 – Naming with Transition Metals
  • can have charges, so you cannot tell the charge based on the it is in.
  • Since transition metals can have charges, we use a to indicate the charge.
  • Review of Roman Numerals

1 =

2 =

3 =

4 =

5 =

  • **You should not use a roman numeral over 5.
  • When compounds that start with a transition metal, you should charges to figure out the of the transition metal.
  • Remember add to the anion if it is not a polyatomic ion.
  • Ex: CuO
  • Sample Problems
  • Write the names for the following:

Cu2O

FeCl3

PbSO4

  • Practice Problems
  • Write the name of the following:

PbS2

Zn(C2H3O2)2

Ag3PO3

  • For the naming system for ______the old names are used with the suffix –ic or –ous.

Ion / Old Name / Ion / Old Name
Fe3+ / ferric / Sn4+ / stannic
Fe2+ / ferrous / Sn2+ / stannous
Cu2+ / cupric / Pb4+ / plumbic
Cu+ / cuprous / Pb2+ / plumbous
Co3+ / cobaltic / Hg2+ / mercuric
Co2+ / cobaltous / Hg22+ / mercurous
  • The ending indicates a charge, and the ending indicates a charge.
  • When writing the for a compound, you figure out the for the transition metal and then find the old name on the .
  • Ex: FeS

Fe+2S-2

Fe+2 = ferrous

FeS = ferrous sulfide

  • Practice Problems
  • Write the old names for the following:

Cu3P

Fe(NO3)3

PbS

  • When writing the for a compound that starts with a , you must ______.
  • Ex: vanadium (V) fluoride
  • REMEMBER THE ROMAN NUMERAL IS THE , NOT THE !!!!!!!!!!!!!!!!
  • Sample Problems
  • Write the formula for the following:

Tin (II) permanganate

Mercury (I) oxide

Cobaltic carbonate

  • Practice Problems
  • Write the formula for the following:

Gold (II) iodide

Vanadium (IV) nitrite

ferrous chromate

  • Section 9.2 Assessment
  • Write the formula for chromium (III) nitrite.