Chemistry Bonding Test

Question 1

a force/mutual electrical attraction that holds atoms together in a substance

Answer 1

chemical bond

Question 2

a measure of the ability of an atom in a bond to attract electrons

Answer 2

electronegativity

Question 3

the tendency of atoms to prefer to have 8 valence electrons

Answer 3

octet rule

Question 4

compound formed when 2 or more elements are covalently bonded

Answer 4

molecule

Question 5

a binary ionic compound between 1 kind of metal atom and 1 kind of nonmetal atom

Answer 5

salt

Question 6

network of cations and anions that are mutually attracted to one another

Answer 6

crystal lattice

Question 7

a compound made of positive and negative ions that chemically bond in a way that the charges equal out

Answer 7

ionic compound

Question 8

charged atoms

Answer 8

ion

Question 9

positively charged atoms from losing electrons

Answer 9

cations

Question 10

negatively charged atoms from gaining electrons

Answer 10

anions

Question 11

a positively or negatively charged, covalently bonded group of atoms

Answer 11

polyatomic ion

Question 12

metals that “transition” because they can form many different ions

Answer 12

transition metal

Question 13

differentiate between the forces between different substances versus the forces within a substance

Answer 13

Intermolecular forces are between different substances. Intramolecular forces are within the same substances (chemical bonds).

Question 14

Explain what is meant by the statement, “Bonding is a spectrum”

Answer 14

There aren’t just two types of bonds. It is a spectrum with ionic and nonpolar covalent at the two extremes.

Question 15

Write a sentence to summarize the connections between chemical bonds, chemical reactions, and compounds.

Answer 15

Chemical bonds form through chemical reactions and result in new compounds

Question 16

Explain why most atoms form chemical bonds and why some atoms don’t.

Answer 16

They form bonds to be stable with full outer energy levels of electrons. Noble gases don’t form chemical bonds because they are already stable.

Question 17

Explain the difference between what a chemical formula tells you about an ionic versus a covalent compound.

Answer 17

In a covalent compound, the chemical formula tells you exactly the number and types of atoms. In an ionic compound, it represents the ratio of cations to anions in the crystal lattice.

Question 18

Create a chart to distinguish between covalent and ionic bonds.

Answer 18

Ionic: Electrons are transferred, Typically between a metal and a nonmetal, always between ions, can result in the formation of a salt
Covalent: Electrons are shared, Always between nonmetals, Can be polar or non-polar, results in the formation of a molecule

Question 19

Create a chart to distinguish the properties of covalent compounds from the properties of ionic compounds

Answer 19

Ionic: crystalline solids, high melting and boiling points, can conduct electricity when dissolved in water
Covalent: can be solid liquid or gas, low melting and boiling points, cannot conduct electricity when dissolved in water

Question 20

Be able to explain what a chemical formula tells you about a compound and predict properties of the compound based on the bonds that hold it together

Answer 20

A chemical formula tells us the number of atoms of each element in a compound. Ionic bond - crystalline solids, high melting and boiling points, etc. Covalent bond - solid liquid or gas, low melting point, etc.

Question 21

Be able to identify a bond or compound as ionic or covalent based on a picture, description, difference in electronegativity, or example.

Answer 21

Ionic transfers, Covalent shares

Question 22

Be able to use an element’s location on the periodic table to predict its oxidation number and bonding tendencies

Answer 22

ex) 1+, 2+, 3+, 4+/-, 3-, 2-, 1-

Question 23

PRACTICE: List the number of atoms of each element in the compounds.
a) AlF^3
b)K^3P
c) Ca(ClO^3)^2

Answer 23

a) Aluminum - 1, Fluorine - 3
b) Potassium - 3, Phosphorous - 1
c) Calcium - 1, Chlorine - 2, Oxygen - 6

Question 24

Explain the connection between electronegativity and the formation of an ionic bond.

Answer 24

The difference in electrognegativity is so great that one atom takes the electrons from the other because it has such a greater attraction to them.

Question 25

Use an example of an ionic compound to explain the “rule of zero change”.

Answer 25

MgCl^2 is one atom of magnesium with a 2+ charge, and two atoms of chlorine, each with a 1- charge. 1(2+) + 2(1-) = 2+ + 2- = 0.

Question 26

DIfferentiate between binary ionic compounds, compounds with polyatomic ions, and binary molecular compounds.

Answer 26

Binary ionic compounds are made of 2 elements that transfer electrons in an ionic bond. Compounds with polyatomic ions are made of one or more covalently bonded charged group of atoms that transfer electrons in an ionic bond. Binary molecular compounds are made of 2 elements that share electrons in a covalent bond.

Question 27

Explain why it is necessary to include a Roman numeral when naming an ionic compound with a transition metal.

Answer 27

You cannot determine the charge of a transition metal from the periodic table, so the Roman numeral is necessary to indicate the charge of the metal ion.

Question 28

Give an example of a common compound and how the properties of the elements that make it up are different from that of the compound itself.

Answer 28

NaCl = sodium chloride
Sodium on its own is extremely explosive when it contact with water.
Chlorine on its own is extremely poisonous.
Together they make table salt, which we can eat.

Question 29

Be able to illustrate the formation of ionic bonds using Lewis structures.

Answer 29

know how to transfer the dots, what causes a bond where the dash forms, etc.

Question 30

Be able to apply nomenclature rules to determine the chemical formula and the name of an ionic compound, including those with polyatomic ions and/or transition metals.

Question 31

Draw the Lewis Structure for the bond that would form between calcium and chlorine. Then write its chemical formula and name.

Question 32

Name the following compounds.
a) Na2CO3
b) NH4C2H3O2
c) BaCl2
d) Mn (OH) 2

Answer 32

a) Sodium carbonate
b) Ammonium acetate
c) Barium chloride
d) Manganese (II) hydroxide

Question 33

Write the chemical formula for the following compounds.
a) Magnesium fluoride
b) Calcium phosphate
c) Gold (II) carbonate
d) Lead (IV) sulfate

Answer 33

a) MgF2
b) Ca3 (PO4) 2
c) AuCO3
d)Pb (SO4) 2