Chemical Bonding

Question 1

Lewis dot diagram

Answer 1

-a diagram to represent the arrangement of valence electrons

Question 2

electron configuratiion

Answer 2

-the number of electrons for an element based on each energy level
-example Neon’s electron configuration is 2,8 (there are 2 electrons on the first energy level and 8 electrons on the second energy level)

Question 3

chemical formula

Answer 3

-a set of chemical symbols and or subscripts that show the elements present in a compound

Question 4

valence electrons

Answer 4

-the electrons on the outer energy level
-they are used to make chemical bonds

Question 5

ionic bond

Answer 5

-a bond formed between a metal and a nonmetal
-the valence electrons a lost and gained

Question 6

covalent bond

Answer 6

-a bond formed between two nonmetals
-the valence electrons are shared

Question 7

metallic bond

Answer 7

-a bond formed between two metals

Question 8

oxidation number

Answer 8

-the number of gained or lost electrons with the new charge

Question 9

ion

Answer 9

-a charged atom

Question 10

cation

Answer 10

-an atom that has lost electrons and now has a positive charge

Question 11

anion

Answer 11

-an atom that has gained electrons and now has a negative charge

Question 12

subscript

Answer 12

-the number in a chemical formula that shows how many atoms are present
-example H2O (the “2” is usually smaller, it shows there are 2 Hydrogen atoms and 1 Oxygen atom in the chemical formula)

Question 13

octet rule

Answer 13

-for an atom to be stable, it must have 8 electrons in the outer energy level (example- Neon has 8 valence electrons= stable, Lithium has 1 valence electron= unstable)
-this makes the energy level “full”
-to be stable the outside energy level must be “full” with 8 valence electrons or “empty” with 0 valence electrons