Unit 7, Chapter 19

Integrated Science

Chapter 19 Learning Goals Relate the chemical behavior of an element, including bonding, to

its placement on the periodic table.

Identify how elements form chemical bonds and the role of electrons in bonding.

Predict the chemical formulas of compounds made up of two different elements.

Write chemical formulas for compounds made up of many different types of elements.

Calculate the formula mass of a compound and compare different compounds based on their formula masses.

Identify the environmental and economic impact of recycling plastics.

Chapter 19 Vocabulary Terms ionic bond

monoatomic ion

octet subscript

polymer

polyatomic ion

react

valence electron

Avogadro number

chemical bond

chemical formula

covalent bond

diatomic molecule

energy level

formula mass

ion

19.1 Bonding and Molecules

Key Question:

Why do atoms form chemical bonds?

*Read text section 19.1 AFTER Investigation

19.1

19.1 Bonding and Molecules The outer electrons are

involved in bonding. These are called

valence electrons. Most stable atoms have

eight valence electrons. (Some have two)

When an atom has 8 valence electrons, it is said to have an octet of electrons.

8

7

6

5

1

2

3

4

19.1 The Octet Rule

19.1 Bonding and Molecules

A sodium atom is chemically unstable because it has only one valence electron.

With the exception of the transition metals, the column of the table tells you how many valence electrons each element has. Columns are called groups.

For example, the atoms of the elements in Group 1A have only one valence electron.

1

If it helps put the valence e- in ()

Group 1 the alkali metals or lithium family

Group 2 the alkaline earth metals or beryllium family

Group 3 scandium family (consisting of the rare earth elements plus the actinides)

Group 4 the titanium family

Group 5 the vanadium family

Group 6 the chromium family

Group 7 the manganese family

Group 8 the iron family

Group 9 the cobalt family

Group 10 the nickel family

Group 11 the coinage metals (not an IUPAC-recommended name) or copper family

Group 12 the zinc family

Group 13 the boron group or boron family

Group 14 the carbon group or carbon family

Group 15 the pnictogens or nitrogen family

Group 16 the chalcogens or oxygen family

Group 17 the halogens or fluorine family

Group 18 the noble gases or helium family or neon family

Lewis Dot StructuresCount the total valence electrons for the

molecule

Figure out how many octet electrons the molecule should have, using the octet rule:— All atoms want 8 except for H and He = 2

If the number is 3 or less atom gives up those negative e-!

If the number is 4 or more atom will gain enough e- to make 8.

19.1 Ionic Bonds Ionic bonds are formed when atoms gain or lose electrons.

Sodium and chlorine form an ionic bond to make sodium chloride (table salt).

19.1 Covalent BondsWhen electrons are shared between two

atoms, a covalent bond is formed.

19.1 Ionic or Covalent Bond? Elements can be

classified as metals, metalloids, and nonmetals.

Generally, bonds between a metal and a nonmetal tend to be ionic in character.

Bonds between two nonmetals can be classified as covalent.

19.2 Chemical Formulas

Key Question:

Why do atoms combine in certain ratios?

*Read text section 19.2 AFTER Investigation 19.2

19.2 Chemical Formulas All compounds

have an electrical charge of zero; that is, they are neutral.

19.2 Oxidation Number

An oxidation number indicates how many electrons are lost, gained, or shared when bonding occurs.

Common Polyatomic Ions

19.3 Comparing MoleculesKey Question:

What is the meaning of a chemical formula?

*Read text section 19.3 AFTER Investigation 19.3

19.3 Comparing Molecules

One atom of hydrogen is 1/12 the mass of a carbon atom.

19.3 Comparing Molecules

19.3 Comparing Compounds The Avogadro number is the

number of atoms in the atomic mass of an element or the number of molecules in the formula mass of a compound when these masses are expressed in grams.

One set of 6.02 x 1023 atoms or molecules is also referred to as a mole of that substance.