Chapter 6-7: Ionic and Metallic Bonding Flashcards
What is the formula for lead(II) nitrate?
Pb(NO3)2
What is the name of the compound Sr(NO2)2?
Strontium nitrite
A regular, repeating, three dimensional array of atoms, molecules or ions that minimizes energy.
Crystal
Using electron dot structures, predict the formula for rubidium phosphide.
Rb3P
What is the formula for nickel(III) sulfide?
Ni2S3
A charged group of covalently bonded atoms.
A polyatomic ion
Which of the following would you expect to have a higher melting point? Why?
KCl or CaCl2
CaCl2 should have the higher melting point. Calcium is a smaller ion than potassium, causing the charges to be closer together, and the lattice energy to be stronger. Additionally, the calcium ion has a +2 charge, but the potassium ion has only a +1 charge. Lattice energies (and thus melting points) are higher for ions having higher magnitude charges.
A rule that states that atoms form compounds in order to achieve 8 valence electrons (a noble gas electron configuration).
The octet rule
The collection of a metal’s delocalized valence electrons that move freely throughout the metal, shared by all of the metal’s cation cores.
Electron sea
What is the name of the compound MgCl2?
Magnesium chloride
A compound composed of only 2 different elements; a monatomic cation and a monatomic anion. Their names always end in -ide.
Binary ionic compound
How many total electrons are there in the phosphide ion, P-3?
18
A chemical bond that results from the electrical attraction between cations and anions.
Ionic bond
What is the name of the compound KOH?
Potassium hydroxide
The chemical bonding that results from the attraction between metal cation cores and the surrounding sea of electrons.
Metallic bonding
The amount of energy as heat required to vaporize a metal. It is a measure of the strength of the bonds that hold the metal together.
Enthalpy of vaporization