Using the formula of a compound. how might we determine whether or not its ionic.

Ions need to have a full octet, if there is two elements that can either be positive or negative then one needs to gain an electron so it can act like the nearest noble gas, while the other needs to lose an electrons. Then they will react and make an ionic compound.

Describe the attractive and repulsive forces that occur as two atoms are brought closer together.

When two atoms are brought closer together the attraction pulls the electrons from one atom with the other atom's nucleus. Then they become balanced because of the repulsive force that makes them have a positive charge when they are pulled together.

Predict the molecular shape of Br2 and Hbr.

They both are linear because they both have only three elements.

Why do ionic compounds ordinarily have such high melting and boiling points?

The reason why ionic compounds have high melting and boiling points is because of their physical properties. When the compound has high heat it will break the bond. For example Sodium chloride is an ionic compound, because of its electrostatic attraction it takes a lot of heat energy. The difference between different copounds depends on the charge and the size of the ion.

Work Cited:
www.chemguide.co.uk/atoms/structures/ionicstruct.html.

What are anions?

They are negatively charged Ions. When naming the element or compound the anion is the second one listed because its a nonmetal. The charges for anions are -1, -2, -3, -4.

What are cations?

Cations are positively charged ions. When naming the element or compound the cation is the first one listed because its more often times a metal. The charges that cations have are +1 , +2 , +3 , +4 .

Are ions stable?

All Ions aren't stable because they need a full even shell to be stable. You can use the Bohr structure to show you the ions are stable.

The electron configurations for...

a. Calcium , Ca.
[ Ar ] 4s2
b. Oxygen , O.
[He] 2s2 2p4
c.) Iodine ,I
 [Kr] 4d10 5s2 5p5
d.) Xenon, Xe
[Kr] 4d10 5s2 5p6

What happens to the stability and energy of two atoms as they form a covalent bond?

Covalent bonds release energy when two atoms come together. This makes the electron more stable.

Work Cited:
www.chacha.com

Compare the behavior of bonding electrons in a non-polar covalent bond with that of bonding electrons in a polar covalent bond.

When a chemical bond is formed the atom will become more stable. It depends on the bond whether it will gain or loose electrons because of the energy it gives off. Ionic bonds have more energy because of the movement between electrons.

Work Cited:
www.science.kennes.edu

How might changing the shape of a molecule affect its properties?

Changing the shape of the molecule effects its properties in many ways such as changing its melting and boiling point and changing how it reacts.

Compare and Contrast Ionic, Covalent and Metallic bonds.

Covalent bonds occur when one or more electrons are joined by two atoms. Ionic bonds occur when one or more of the electrons are attached to another atom, or are removed. When that happens it creates positive and negative ions that can join with each other. Metallic bonds happens between metals, they share unplaced electrons. In the valence shell of metal atoms they have a small amount of electrons.

Work Cited:
http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/bond.html

Explain the forces that hold the bonds together

The Chemical bond is attracted and happens between molecules and atoms that have two or more atoms. Electromagnetic forces between different charges occurs between electrons and the nuclei. Metallic bonding happens between two electrons called delocalized, and conduction. Metallic bonding can be compared to some salts. Metallic bonding is the physical properties like the conductive of thermal and electric,luster and strength. With ionic bonds one element has a negative charge and the other has a positive. This is called an electrostatic attraction because its both a positive and negative charge.

Work Cited:
http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/bond.html