Honors Chemistry Unit 3 Review

Ionic

Forms when atoms are held together by the attraction between opposite charges, when charge ions of metal and nonmetal attract, one loses one or more of their electrons (complete transfer of electrons)

metal, nonmetal

Ionic bonds are made of ___ and _____ elements

0

In forming an ionic compound, the overall charges must be equal to ___

solid

Ionic bonds are always (solid/liquid/gas) at room temperature

do

Ionic bonds (do/do not) have a lattice structure

high, hard

Ionic bonds have a (high/low) boiling point because it is (hard/easy) to separate positive and negative ions in the lattice structure

when dissolved, free

Ionic bonds are conductive only ____ _____ because then they are (free/unable) to move past each other

more

Ionic bonds are (more/less) likely to be soluble in water

always crystalline, hard, do not, brittle

The physical characteristics of ionic bonds are that they’re (always/never) crystalline, (hard/not as hard) because the bonds (do/do not) want to come apart, and (soft/brittle)

Covalent

shared electrons end up between the two bonded nuclei

nonmetal

Covalent bonds are made with two ______ atoms

may be, both liquid and gas

Covalent bonds (may be/ are never) solid at room temperature, but can also be (liquid/gas/both liquid and gas) at room temperature

isn’t

There (is/isn’t) a lattice structure in covalent bonds

longest and weakest, strongest and shortest

Covalent bonds can be single (longest and weakest/strongest and shortest), double, or triple (longest and weakest/strongest and shortest)

weaker, lower

Covalent bonds are (weaker/stronger) than ionic bonds, so they have a (higher/lower) melting and boiling point

do not, charge, free

Covalent compounds (do/do not) conduct electricity because there are no ___ particles (free/not free) to move.

less

Covalent compounds are (more/less) likely to be soluble in water

may be, aren’t, aren’t as hard and brittle

The physical appearance of covalent bonds are that they (may be/always are) crystalline but frequently (are/aren’t), and they aren’t as (hard and brittle/soft and malleable) 

no

Do covalent bonds have a lattice structure?

Metallic

Sea of electrons: “free floating” valence electrons between all the metal cations (metal nuclei and non-valence electrons)

solid

At room temperature, metallic bonds have a ____ state of matter

metals

The type of atoms that are in metallic bonds are ____

yes

Do metallic bonds have a lattice structure?

cations, wire, sea of electrons can move

How are metallic bonds ductile?

When the metal ____ are pulled into a ___ shape, the ___ __ ____ can ___ and split into spaces

sea of electrons, free, electricity

How are metallic bonds conductive?

The electrons in the ___ ___ ____ are ____ to move throughout the compounds, which allows ____ to flow

cations, closer, sea of electrons, fill in

How are metallic bonds malleable?

The metal _____ can move ____ together and form any shape.The ___ ___ _____ will ___ ___ between the cations in any shape.

high

Metallic bonds have a (high/low) melting point

Polyatomic

Single ion with multiple atoms

Polar

UNEQUAL sharing of electrons

Nonpolar

EQUAL sharing of electrons

cannot

Ionic bonds (can/cannot) be examined for polarity

Dipole

shows direction electrons are pulled in covalent bond

within

INTRAmolecular forces are ____ a compound

ionic, covalent, metallic

Examples of INTRAmolecular forces are ___, _____, and _____

between

INTERmolecular forces (IMF’s) are attractions _____ two or more molecules

Hydrogen bonds, Dipole Dipole, London Dispersion Forces

Examples of intermolecular forces are ______, _____ _____, and ______ _____ _______

Hydrogen bonds

when a H atom of 1 molecule is attracted to a highly electronegative atom (F, O, N)

Dipole Dipole

attractions between oppositely charged regions of a POLAR molecule

London Dispersion Forces

induced dipole dipole between nonpolar molecules

weakest, strongest

London Dispersion Forces are the (strongest/weakest) and hydrogen bonds are the (strongest/weakest)

London Dispersion

Nonpolar molecules only have what type of IMF?

London Dispersion, dipole-dipole

Polar molecules have what types of IMF’s?

all

Polar molecules with H-N, H-F, H-O bonds and lone pairs of e^- have what types of IMF’s?

VESPR

Physical 3D shape of covalent molecules