Ionic/Metallic Bonding

Question 1

Compounds are held together by _______ bonds

Answer 1

chemical

Question 2

An attractive force between the atoms that holds them together

Answer 2

bond

Question 3

Atoms form bonds to _______ themselves by lowering their chemical potential energy

Answer 3

stabilize

Question 4

three main types of bonds

Answer 4

ionic, covalent, and metallic

Question 5

in ionic bonding, electrons are completely ________ from a metal to a non-metal

Answer 5

transferred

Question 6

when reacting atoms either lose or gain negatively charged electrons, they form _______

Answer 6

ions

Question 7

a metal forms a ______

Answer 7

cation

Question 8

a non-metal forms an ______

Answer 8

anion

Question 9

oppositely charged ions are attracted to each other by ________ forces

Answer 9

electrostatic

Question 10

ionic compounds don’t exist as ________

Answer 10

molecules

Question 11

ions attract one another from all ________ with each ________ ion surrounded by negative ions and each ________ ion surrounded by positive ions

Answer 11

directions; positive; negative

Question 12

a crystal ______ is caused by a regular, repeating, three-dimensional ______ of alternating positive and negative ions

Answer 12

lattice; pattern

Question 13

the _______ of cations to anions is constant throughout the crystal lattice

Answer 13

ration

Question 14

the ______ number of atoms in the crystal will vary depending on its ______

Answer 14

total; size

Question 15

when we write chemical formula for an ionic compound we only write the ______ of the ions

Answer 15

ratio

Question 16

Melting Point: very high (a large amount of energy must be put in to overcome the strong electrostatic attractions and separate the ions)
Strength: very brittle (any dislocation leads to the layers moving and similar ions being adjacent. the repulsion splits the crystal)
Electrical: don’t conduct when solid- ions held strongly in the lattice conduct when molten or in aqueous solution; the ions become mobile and conduction takes place
Dissolving an ionic compound in water breaks up the structure so ions are free to move to carry electricity

Answer 16

physical properties of an ionic compound

Question 17

bonds between two or more metal atoms

Answer 17

metallic bonding

Question 18

metals have different properties from ____ or ______ solids

Answer 18

ionic; covalent

Question 19

metals have a low _____ electron number

Answer 19

valence

Question 20

electrons are allowed to roam ______ in the overlapping orbitals

Answer 20

freely

Question 21

the electrons are _________, meaning they don’t belong to any one atom. this creates a “sea of electrons” that surround the metal atoms that are packed in a crystal lattice structure

Answer 21

delocalized

Question 22

metals atoms are held in place because all the valence electrons are _______________ attracted to all of the metal atoms

Answer 22

electrostatistically

Question 23

metals are held tightly in place because of _______________. this causes metals to have a _____ melting point

Answer 23

electrostatic attractions; high

Question 24

most of the unique properties of metals are due to the _______ electron sea

Answer 24

mobile

Question 25

since the electrons can move freely, metals are very __________

Answer 25

conductive

Question 26

electrons can also move to a large number of energy states, therefore they can absorb and release many _________ of energy

Answer 26

wavelengths

Question 27

re-releasing many different wavelengths of light make the metals appear ______

Answer 27

shiny

Question 28

unlike ionic bonds, metallic bonds are ______________, so atoms can slide past each other without the crystal lattice ________ apart

Answer 28

non-directional; breaking

Question 29

metal ions are attracted to the sea of electrons, not to each other. this is why metals are very ________ and ________

Answer 29

ductile; malleable