Unit 2 AP Chemistry Mrs. Coleman 10/19/26 well the keys are an ionic compound structures and properties

Where are covalent bonds formed?

Between two nonmetals sharing electrons

how are ionic bonds formed

When a metal transfers, electrons to a nonmetal in the opposite charges attract

The greater the electronegativity difference between two atoms

The more polar the bond becomes

what types of reactions make CO2 and H2O?

Combustion

how many bonds does carbon make in a compound?

four

109.5 degrees

4 domains

120°

three domains

180°

Two domains

hybrid orbital 4 domains

SP3

hybrid orbital three domains

SP2

hybrid orbital two domains

SP

what happens in asymmetrical molecules?

Dipoles do not cancel

dipoles do not cancel in

polar molecules

what happens in symmetrical molecules?

dipoles cancel

if dipoles canceled

non-polar molecule

Sigma

Single bond

Sigma plus pi

Double bond

Sigma +2 pi bonds

Triple bond

lattice energy

Energy to break an ionic bond in a compound

Lattice energy increases as

The Ions Charge increase

lattice energy decreases as (coulomb’s law)

radii of the ions increase

comparing the number of valence electrons to the number of electrons around it in the structure

Formal charge

formal charge

Valence electrons- lone pair electrons - 1/2 bonding electrons

when drawing Louis.structure what should you do first

Obey octet Rule Then use formal charge

Bond between metals

Metallic

metallic bonds

always conduct electricity and have varied hardness

Interstitial alloys are made when

smaller atoms fits into the gaps between the larger atoms of a metal metallic crystal

substitutional all alloys are made when

The radii of the medals are similar to size and are substituted into the crystal lattice

Chemical bonds

Have attraction between nucleus of atoms

Bond polarity

Difference in electronegativity ( values of two elements.)

linear

180*

sp

linear

1

linear

trigonal planar

120*

sp2

trigonal planar

sp3

tetrahedral

bent

<120*

tetrahedral

109.5*

trigonal pyramidal

<109.5*

bent with two lone pairs

<109.5*

2

trigonal planner

3

bent

4

tetrahedral

5

Trigonal Pyramidal

6

bent

The presence of pi Bonds means that

Bones are unable to rotate which leads to geometric isomers

geometric isomers

Have the same atoms, but have different arrangements and are not super impossible

as a number Of bonds between two atoms increase

The bond increases and strength and energy, but decrease decreased in length

formula for bond length

Number of bonds divided by the number of atoms connecting to it (so if the molecule had 3 atoms not in a ring and 2 double bonds (CO2) then bond length wld be 3/2)

when electrons Are shared in a covalent bond the shared electrons spend more time around

The more an electronegative element in the bond (gives them more electronegative element a partial negative Charge)

to know if a molecules polar, you need to know

If the bonds are polar and the overall shape of the molecule

difference in electronegativity between two atoms can be measured by

The absolute value of Their subtracted masses

High melting and boiling points and solids at room temperature brittle

Ionic bonds because a lot of attractive forces Needed to break to make liquid, which takes a lot of energy

ionic bonds

Poor conductors when solid, good conductors when molten or aqueous(Dissolved in water)

why are ionic bonds good conductors when they're molten or aqueous

makes it able to Move freely

what does conductivity require?

Charge particles and freely moving ions

two more nonmetals that share electrons have a

Covalent bond

covalent bonds can

share equally which is nonpolar and has a very small Electronegativity difference

Share unequally polar, which has a mid to large electronegativity difference

covalent bonds have a —- Melting and boiling point

Low

why can covalent bonds be solid liquid or gas at room temp

There are only a few attractive points and not a crystal structure

covalent bonds are ——- Conductors of electricity

Poor because they don't make ions/don't have charge particles

how to determine Bond polarity

look at PT and see distance between the further away on PT the more polar they are or use F O N Cl Br I S C H fluorine , oxygen, nitrogen, chlorine, bromine, iodine, sulfur, carbon hydrogen

dipole moment

Shows the Direction of the charge separation and always points towards the more Electro negative atom

de localized electrons/ sea of electrons/ Electrons are free floating

metallic bonds

in a metallic solid

Violence elections are free to move throughout the entire

in metallic bonds

Electrons are equally shared, and are not associated with a single atom

good conductors because of charge particles and free flowing

metallic bonds

metallic bonds have —— Melting/boiling points

High because lots of points of attractions between positives and negatives (exceptions, mercury and gallium)

metallic bonds are

Malleable and ductile which means they are capable and can be drawn into wires because it's not rigid everything just flows like a car frame In a crash

alloys

Mixture of two or more elements primarily metals

why do alloys easily form?

Because replacing atoms does not greatly disturbed the metallic bonding

substitutional alloy

One atom is replaced by another usually atoms of similar atomic radius often strengthens, but s Still remains malleable

interstitial alloys

atoms are added into the spaces between other atoms usually one atom is significantly smaller than the other much stronger, but less malleable

if pico meters up two elements are almost the same or same

it's a Substitutional alloy (If they are very different, it's interstitial)

bonding is based on

The bounds between attractive and repulsive forces (Attraction between Nucleus and proportion of electrons)

Energy required to break a bond endothermic (energy in) or energy release during the formation of a bond exothermic ( energy out

bond energy

Atoms separated

No attraction

for potential energy curve of a covalent bond bottom of curve is the

Optimal distance to maximize the attraction/the most stable bond length/largest bond energy

for potential energy curve of a covalent bond left of bottom of curve

atoms are too close Repulsion dominates

every bond is

Two electrons

ionic bonds

F equals (Q1Q2)/R2

when comparing ionic bonds

If no difference in charges look at size And if same size look at church

High lattice energy

High melting point

which Trump's charge or size

size

octect rule

elements need eight beyond electrons to fill S&P orbitals except eight, which forms a duet -2 electrons

Hypervalent or expanded octet

adam's. Three and above can use the orbitals, so Otte can expand to have more than eight electrons on the central atom.

electron deficient atoms (hypovalent)

boron and beryllium form molecules with the less stable octect

resonance structures

Bonding same

formal charges used when

Greater than one Valid lewis structure is possible

formal charge =

ve - nonbinding e. -1/2 bonded e

there's no like charges next to each other for

Formal charges

more electrical negative atom is

Most negative

overall charge should be—- Or charge of ion for formal charge

Zero