1. The Structure of Matter
Section 1 – Compounds and Molecules
Section 2 – Ionic and Covalent Bonding
Section 3 – Compound Names and Formulas

2. State Standards
CLE – Distinguish between common ionic and covalent compounds
CLE – Construct chemical formulas for common compounds
CLE.3202.TE.4 – Describe the dynamic interplay among science, technology, and engineering within living, earth-space, and physical systems

3. 1 – Compounds and Molecules
KEY QUESTIONS
What holds a compound together?
How can the structure of chemical compounds be shown?
What determines the properties of a compound?

4. Chemical Bonds
Forces that hold atoms or ions together in a compound are chemical bonds
H and O form bonds when water is formed

5. Chemical Structure
The way that atoms are bonded together to make a compound results in chemical structure
This structure can be shown by various models
Example : Ball and Stick Model

6. Chemical Structure Some models show bond length and bond angles
Ball and stick
Other models show space occupied by compounds
Space-filling model ( Figure 2 in Chapter 6 – page 178 )
ETHANOL 

7. Bonds are like SPRINGS Bonds are flexible and act like springs
Bonds can bend, stretch, compress, and twist
Do this without breaking
Temperature affects this motion ( Kinetic Theory )

8. How Structure Affects Properties
Chemical structure determines properties
Network structures form strong solids
Quartz ( network of rigid Si-O-Si bonds )
Have to break network to split up
Some networks consist of bonded ions
Salt ( NaCl formed from Na+ and Cl- ions )
Group 1 elements form cations / Group 17 anions
Some materials are made of separate structures
Sugar is a group of single ( the same ) molecules
Can pull out single molecules unlike with a network

9. Attractive Forces Vary
Example : H2O
Water is liquid at room temp
Sugar is solid at room temp
Indicates that water has weaker attractive forces

10. Attractive Forces Vary
Forces between molecules
Example : H2O
Water has higher boiling point than H2S
Indicates that water has stronger attractive forces

11. 1 – Compounds and Molecules
KEY QUESTIONS
What holds a compound together?
How can the structure of chemical compounds be shown?
What determines the properties of a compound?

12. 2 – Ionic and Covalent Bonding
KEY QUESTIONS
Why do atoms form bonds?
Why do ionic bonds form?
What do atoms joined by covalent bonds share?
What gives metals their distinctive properties?
How are polyatomic ions similar to other ions?

13. Why do Chemical Bonds Form?
In general, atoms join to form bonds so that each atom may have a stable electron configuration
They want a full level of valence electrons!!

14. Ionic Bonding Formed from the attraction between ions
Ions are formed by transfer of electrons
Na and Cl form salt
Ionic compounds form as networks
Solids are the result
Ionic compounds dissolved in
water conduct electricity

15. Covalent Bonds These are formed when electrons are SHARED
EXAMPLES : O2, Cl2, N2
Atoms may share more than one pair of electrons
Atoms do not always EQUALLY SHARE electrons

16. Metallic Bonds A type of covalent bond Occurs between metals
Electrons move freely between
metal atoms
Metals are flexible and conduct electricity well because their atoms and electrons can move freely throughout the packed structure

17. Polyatomic Ions
Acts as a single unit in a compound, like ions that consist of a single atom do ( like Cl, Na )
Hydroxide ( OH - )
NaOH
Carbonate ( CO3 2- )
CaCO3
Ammonium Sulfate : (NH4)2SO4

18. Polyatomic Ions
Some of these are named based on the number of oxygen atoms in compound
Nitrate vs Nitrite
NO3- vs NO2-
Chlorate vs. Chlorite
ClO3- vs ClO2-

19. 2 – Ionic and Covalent Bonding
KEY QUESTIONS
Why do atoms form bonds?
Why do ionic bonds form?
What do atoms joined by covalent bonds share?
What gives metals their distinctive properties?
How are polyatomic ions similar to other ions?

20. 3 – Compound Names & Formulas
KEY QUESTIONS
How are ionic compounds named?
What do the numerical prefixes used in naming covalent compounds tell you?
What does a compound’s empirical formula indicate?

21. Naming Ionic Compounds
Ionic compounds are named based on the constituent ions
Cations ( + ) are named based on the element
“calcium”
“magnesium”

22. Naming Ionic Compounds
Anions ( - ) are altered names of elements
“oxide”
“chloride”

23. Put ‘Em Together sodium chloride ( NaCl ) magnesium chloride ( MgCl2 )
aluminum oxide ( Al2O3 )

24. Formula Unit sodium chloride ( NaCl ) magnesium chloride ( MgCl2 )
aluminum oxide ( Al2O3 )
calcium fluoride ( CaF2 )
Wikepedia.org

25. Naming Ionic Compounds
Charge ( + ) of many transition metals varies
Fe may have 2+ or 3+
Thus, some names show cation charge
iron(III) oxide [common form ]
iron(II) oxide
Can also see charge in chemical formulas
Fe2O3 [ Fe3+ since Oxygen is often O2- ]
FeO [ both ions have a ‘2’ charge ]

26. Naming Covalent Compounds
Numerical prefixes indicate chemical formula when more than atom is involved
Examples:
carbon dioxide ( CO2 )
silicon dioxide ( SiO2 )
boron tetrafluoride ( BF3 )
Dinitrogen tetroxide ( N2O4 )
N2O4 via Wikepedia.org

27. Empirical Formulas
Indicates the smallest whole-number ratio of atoms in a compound
Some are same as chemical formula
Hydrogen Peroxide is exception:
Chemical Formula – H2O2
Empirical Formula – HO
Formaldehyde, acetic acid, and glucose have same empirical formula

28. Empirical Formula Molecular Formulas ( had Formula Unit for Ionics )
Emprirical formula can be determined by analyzing mass of each element in a compound

29. 3 – Compound Names & Formulas
KEY QUESTIONS
How are ionic compounds named?
What do the numerical prefixes used in naming covalent compounds tell you?
What does a compound’s empirical formula indicate?