1. Atoms and Bonding
Chapter 5

3. Atomic Structure and the Periodic Table
Review the structure of the atom
Protons?
Neutrons?
Electrons?
Nucleus?
Electron Cloud?

4. electron clouds
nucleus

5. Protons (+) Neutron (0) Valence electrons Electron (-) P+ N
A simplified slide
Neutron (0)

6. Atomic Structure and the Periodic Table (cont)
Electrons (negative) move around the nucleus in the electron cloud. The electron cloud has different energy shells (or orbits). In a neutral atom the number of electrons equals the number of protons.

8. Atomic Structure and the Periodic Table (cont)
Valence electrons are the electrons in the outer shell.
The valence electrons determine which elements combine to form compounds!

9. Why do Elements Form Compounds?
1. Atoms combine to complete the outer energy shell of electrons
2. A complete outer energy shell is stable. (atoms with filled outer energy shells won’t combine with other atoms)

10. Why do Elements Form Compounds?
3. shell #1 it is complete with 2 electrons.
4. Shells # 2-7 are “complete” with 8 electrons

12. What happens when a chemical bond is formed?
A chemical bond is the force of attraction that holds atoms together
A new substance is formed in a chemical reaction
properties of the new substance are different than the properties of the elements that make them up
Electrons are gained, given away or shared

13. Electron Dot Diagrams Shows valence electrons only
Uses dots to represent electrons
Can be used to show how elements bond

14. Chemical Formula
Chemical Formula - A shorthand way to write the name of the compound
What information does a chemical formula contain?

15. Metals
METALS are on the left side of the Periodic Table. They have a low number of valence electrons and can easily give them to other atoms.
Almost empty shells

16. Nonmetals
B. NONMETALS are on the right side of the Periodic Table. They have a high number of valence electrons and can easily take or share valence electrons from other atoms
Almost full shells

17. Semi Metals
C. SEMIMETALS are found between metals and nonmetals along the zigzag line. They can either lose or share valence electrons with other atoms
About half full shell

19. Ionic Bonds
ION- a charged particle; atoms either gain or lose electrons to form:
A. Positive Ions form when atoms lose electrons (more protons than electrons)
B. Negative Ions form when atoms gain electrons (more electrons than protons)

20. Ionic Bonds Metal to nonmetal
Transfer of electrons from one atom to the other

22. How does an ionic bond form?
1.Metals lose electrons and form positive ions. Nonmetals gain electrons and form negative ions.
2. Ions with opposite charges attract each other (+ and – attract)

23. Properties of ionic compounds
Very strong bonds
Form crystal lattice (alternating, repeating)
hard, brittle
solids with high boiling and melting points,
conduct electricity when dissolved in water.

25. Naming Ionic Compounds
name the positive ion (metal) first
name the negative ion (nonmetal) next with the ending changed to –ide
NaCl:
sodium + chlorine = sodium chloride

26. Name these: K2S: Potassium + sulfur = potassium sulfide Li2O:
lithium + oxygen = lithium oxide
Mg3P2
Magnesium + phosphorous =
magnesium phosphide

27. Covalent bonds
Form nonmetal to nonmetal
Shared electrons

28. How does a covalent bond form?
atoms share electrons to fill outer energy shells (it takes too much energy to transfer electrons)
the force that holds atoms together in a covalent bond is the attraction of each atom’s nucleus for the shared pair of electrons

29. Properties of covalent compounds
Weak bonds
low melting & boiling points
Many are gases and liquids
cannot conduct electricity when dissolved in water

30. molecule
a neutral group of atoms held together by a covalent bond; smallest piece of a compound
Covalent compounds are also called molecular compounds

32. Diatomic Elements:
An element that bonds with itself to form the simplest of molecules.
There are only 7 elements that are diatomic.
H, N, O, F, Cl, Br, I

33. Covalent bonds:

34. XI. Naming covalent compounds
Use prefixes:
Mono = 1
Di = 2
Tri = 3
Tetra = 4
Penta = 5
Hexa = 6

35. Carbon dioxide
CO2
Carbon monoxide CO
Dihydrogen monoxide
H20

36. Metallic Bonds
metal to metal
Positive metal ions “swimming” in sea of released electrons

37. How does a metallic bond form?
Metals tend to lose electrons and form positive ions.
The bonds are held together by the force of attraction between positive metal ions and the many electrons surrounding them.

38. Metallic bond
metal atoms combine in regular patterns which allow the electrons to move from atom to atom

39. Alloy mixture of 2 or more elements, at least 1 is a metal
stronger and less reactive than pure metals.
Properties of alloys are different from the pure metals that make them up

40. Metallic bond: mixture or chemical bond (honors slide)
Alloys are a mixture because they can be in any ratio
Alloys are like a chemical bond because they have different properties than the metals that form them
Alloys are like a chemical bond because the electrons are interacting

41. Properties of Metals Dense shiny
Solids at room temperature (except Mercury)
malleable
ductile
Good conductors of heat and electricity

43. Number scratch paper from 1-10
Cross out number 8
Write the answer to fill in the blank