In many compounds, atoms in main-group elements form ions so that the number of electrons in the outermost energy levels of each ion is _____.
How many more electrons does nitrogen need to have an electron configuration similar to neon?
Atoms of copper and iron _____.
Tend to form cations.
An ion with a negative charge is called a(n) _____.
The lattice energy is a measure of the strength of an _____ bond.
The melting points of ionic compounds are higher than the melting points of molecular compounds because attractive forces between ions are _____ that the attractive forces between molecules.
In a crystal of an ionic compound, each cation is surrounded by _____.
What is the ratio of cations to anions in a compound of sodium ions, Na+, and carbonate ions, CO3 2-?
2 to 1.
The indium(II) ion and indium(III) ion have charges of _____ and _____, receptively.
2+ and 3+.
The symbol HCO3-, represents a _____ ion.
What is the formula for the compound formed by aluminum(III) and SO4 2-?
What is the formula for the compound formed by Ba 2+ and OH-?
Name the compound Ni(ClO3)2.
Nickel (II) chlorate.
Name the compound Fe(NO2)2.
Name the compound CuCO3 -.
The electrons involved in the formation of a covalent bond are _____.
The chemical bond formed when two atoms share one or more pairs of electrons is a(n) _____ bond.
A covalent bond forms when the attraction between two atoms is balanced by repulsion and the potential energy is _____.
At a minimum.
An ionic bond is most likely to form between two elements that have a difference in electronegativity values of _____.
A polar covalent bond is most likely to form between two elements that have a difference in eleectronegativity values of _____.
The correct Lewis structure for the oxygen atom has _____ pairs of valence electrons and _____ single valence electrons.
Two and two.
Do draw the Lewis structure of the polyatomic ion, ClO3 -, you would have to _____ those in the structure of Cl, O, O, and O.
Add one electron to.
In a double bond, two atoms share a total of _____ electrons.
What is the total number of atoms needed to form a tetrahedral molecule?
According to VSEPR theory, which of the following shapes is possible for molecule with the molecular formula of AB2E2? (Linear, Bent, Trigonal Pyramidal)
According to VSEPR theory, which of the following shapes is possible for a molecule with the molecular formula of AB3? (Linear, Trigonal Planar, Tetrahedral)
To indicate resonance, a _____ is placed between a molecule's resonance structures.
A molecule or part of a molecule that contains both positively and negatively charged regions is called a(n) _____.
If the difference in electronegativity values between two elements is 0.1, they will most likely form a(n) _____ covalent bond.
If the difference in electronegativity values between two elements is 1.3, they will most likely form a(n) _____ covalent bond.
Bonds that result in the attraction between the electrons in the outermost energy level of each metal atom in a solid substance and all of the other atoms in the metal are classified as _____ bonds.
A nonbonding pair of electrons in the valence shell of an atoms is called a(n) _____.
A covalent bond in which two atoms share one pair of electrons is called a _____ bond.
A covalent bond in which two atoms share two pairs of electrons is called a(n) _____ bond.
A theory that predicts some molecular shapes by using the idea that pairs of valence electrons surrounding an atoms repel each other is called the _____.
VSEPR theory is short for valence shell electron pair _____ theory.
VSEPR theory predicts that the molecular shape of CBr4 is classified as _____.
VSEPR theory predicts that the molecular shape of NH3 is classified as _____ pyramidal.
Name the compound Sb2S3.
Name the compound P2Se5.
Name the formula of molybdenum hexafluoride.
Name the formula of dipotassium pentasulfide.
What is the chemical formula for the compound cobalt(III) oxide.
What is the chemical formula for the compound tin(II) phosphate.