Chemistry Bonding Test Flashcards
a force/mutual electrical attraction that holds atoms together in a substance
chemical bond
a measure of the ability of an atom in a bond to attract electrons
electronegativity
the tendency of atoms to prefer to have 8 valence electrons
octet rule
compound formed when 2 or more elements are covalently bonded
molecule
a binary ionic compound between 1 kind of metal atom and 1 kind of nonmetal atom
salt
network of cations and anions that are mutually attracted to one another
crystal lattice
a compound made of positive and negative ions that chemically bond in a way that the charges equal out
ionic compound
charged atoms
ion
positively charged atoms from losing electrons
cations
negatively charged atoms from gaining electrons
anions
a positively or negatively charged, covalently bonded group of atoms
polyatomic ion
metals that “transition” because they can form many different ions
transition metal
differentiate between the forces between different substances versus the forces within a substance
Intermolecular forces are between different substances. Intramolecular forces are within the same substances (chemical bonds).
Explain what is meant by the statement, “Bonding is a spectrum”
There aren’t just two types of bonds. It is a spectrum with ionic and nonpolar covalent at the two extremes.
Write a sentence to summarize the connections between chemical bonds, chemical reactions, and compounds.
Chemical bonds form through chemical reactions and result in new compounds
Explain why most atoms form chemical bonds and why some atoms don’t.
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.
Explain the difference between what a chemical formula tells you about an ionic versus a covalent compound.
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.
Create a chart to distinguish between covalent and ionic bonds.
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
Create a chart to distinguish the properties of covalent compounds from the properties of ionic compounds
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
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
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.
Be able to identify a bond or compound as ionic or covalent based on a picture, description, difference in electronegativity, or example.
Ionic transfers, Covalent shares
Be able to use an element’s location on the periodic table to predict its oxidation number and bonding tendencies
ex) 1+, 2+, 3+, 4+/-, 3-, 2-, 1-
PRACTICE: List the number of atoms of each element in the compounds.
a) AlF^3
b)K^3P
c) Ca(ClO^3)^2
a) Aluminum - 1, Fluorine - 3
b) Potassium - 3, Phosphorous - 1
c) Calcium - 1, Chlorine - 2, Oxygen - 6
Explain the connection between electronegativity and the formation of an ionic bond.
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.
Use an example of an ionic compound to explain the “rule of zero change”.
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.
DIfferentiate between binary ionic compounds, compounds with polyatomic ions, and binary molecular compounds.
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.
Explain why it is necessary to include a Roman numeral when naming an ionic compound with a transition metal.
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.
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.
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.
Be able to illustrate the formation of ionic bonds using Lewis structures.
know how to transfer the dots, what causes a bond where the dash forms, etc.
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.
Draw the Lewis Structure for the bond that would form between calcium and chlorine. Then write its chemical formula and name.
Name the following compounds.
a) Na2CO3
b) NH4C2H3O2
c) BaCl2
d) Mn (OH) 2
a) Sodium carbonate
b) Ammonium acetate
c) Barium chloride
d) Manganese (II) hydroxide
Write the chemical formula for the following compounds.
a) Magnesium fluoride
b) Calcium phosphate
c) Gold (II) carbonate
d) Lead (IV) sulfate
a) MgF2
b) Ca3 (PO4) 2
c) AuCO3
d)Pb (SO4) 2
