Chpt. 8, Ionic Compounds and Metals Flashcards Preview

GuchChem > Chpt. 8, Ionic Compounds and Metals > Flashcards

Flashcards in Chpt. 8, Ionic Compounds and Metals Deck (20):
1

ionic bonds

There is no such thing! Ions (ionic compounds) are held together by electrostatic forces, not by bonds. Many people refer to it as ionic bonds anyways, they just don't sound educated.

2

ionic compound

a bond in which positively charged cations are attracted to negatively charged anions due to their opposing charges

3

ionic crystals

more than two atoms typically combine with each other to form larger ionic crystals; the pattern in which the ions arrange themselves is called a crystal lattice

4

unit cell (of a compound)

the smallest repeating unit that makes up a crystal lattice

5

crystal lattice

the pattern in which the ions arrange themselves

6

properties of ionic compounds

hard, brittle, high melting and boiling points, conduct electricity when melted or dissolved

7

Why are ionic compounds hard?

The great resistance to movement that comes are a result of the attraction between their positive and negative charges makes them hard.

8

Why are ionic compounds brittle?

The ions in a crystal lattice are lined up precisely, and unless they remain in exactly that configuration, they become very unstable and will shatter. When subjected to force, the ions will often move relative to one other, and will no longer be in the necessary, precise position.

9

Why do ionic compounds have high melting and boiling points?

The strong electrostatic forces that occur as a result of the attraction between cations and anions is such that they must be subjected to a relatively large amount of energy to break them apart.

10

Why do ionic compounds conduct electricity when melted or dissolved?

Moving ions are one way in which electricity can be conducted, and when ionic compounds are either melted or dissolved, they are free to move around.

11

components of the name of an ionic compound

the first name of the compound names the cation, or positively charged ion (t looks like a plus sign, for positive)

2nd comes the anion, or negatively charged ion in the molecule

for any given compound, the charges on the anion and cation must balance out; some elements have multiple types of cations or anion, and these must be memorized

12

Roman numerals

Roman numerals can be used to indicate the specific positive charge on the cation in cases where the cation may have multiple possible positive charges; the value of the numeral corresponds to the actual charge in the given instance

Roman numerals = (anion charge)(#of anions) / (# of cations)

13

common polyatomic ions, 1-4, (#) = superscript

NH4(+1) = ammonium
NO2(-1) = nitrite
NO3(-1) = nitrate
OH(-1) = hydroxide

14

common polyatomic ions, 4-8, (#) = superscript

CN(-1) = cyanide
MnO4(-1) = permanganate
HCO3(-1) = bicarbonate
C2H3O2(-1) = acetate

15

common polyatomic ions, 9-13, (#) = superscript

CH3COO(-1) = acetate
CO3(-2) = carbonate
SO3(-2) = sulfite
SO4(-2) = sulfate
PO4(-3) = phosphate

16

Electron Sea Theory

a theory in which positively charged metal nuclei are the islands in a "sea" of electrons

17

delocalized electrons

in electrons in the Electron Sea Theory that are not stuck to any specific atom, but can move between the metal nuclei at will

18

alloys

mixtures in which the main component is a metal

19

substitutional alloy

a type of alloy that occurs when the atoms from one element replace those of another (in the lattice structure)

20

interstitial alloys

a type of alloy that occurs when the atoms from one element stick in between the atoms of the other element (in the lattice structure)