Bonding

Front 1

Describe a Molecular Covalent Bond and Cmpds

Back 1

This is a non-metal bonded to a non-metal via the sharing of electrons. The cmpds are further held tother via IMFs. These molecules will have lower MP and BPs due to weak IMFs.

Front 2

Describe Network Solids

Back 2

Quartz (SiO2) or Diamond (pure C) held together via covalent bonds (internally and externally - picture a lattace).

Front 3

Describe Ionic Bonds and Ionic Cmpds

Back 3

AKA Ionic Crystals/Crystalline Salts. A metal bonded with non-metal. Bond formed via the transfer of electrons. Very high MP and BPs. Solids don’t conduct electricity, but liquids and aq. sol’ns do.

Front 4

Describe Metalic Bonds

Back 4

They form metal lattices. Covalent bonds, but outer electrons are very loose. This is why metals can conduce electricity and heat. Metals are ductile (can be drawn into wires), malleable (drawn into sheets), and shiny (luster). Usually have a high MP and BP.

Front 5

What is a Coodinate Covalent bond?

Back 5

When one atom provides BOTH electrons for the bond. The other atom doesn’t provide any electrons. The donor is a Lewis Acid (ligand) and the receiver is a Lewis Bas (Metal Ion).

Front 6

Which elements form diatomic gases?

Back 6

H, N, O, F, Cl, Br, I

Front 7

How does H violate the Octet Rule?

Back 7

It only wants its s shell filled, it has 1 electron prefers 2 max, will make 1 bond.

Front 8

How does Be violate the Octet Rule?

Back 8

It only wants its s shell filled, it has 2 valance electrons which it will share to make 2 bonds.

Front 9

How does B and Al violate the Octet Rule?

Back 9

It has 3 valance electrons which it will share to make three bonds.

Front 10

How do Period 3 and higher elements violate the Octet Rule?

Back 10

They can (but don’t have to) hybrize their p with the d orbitals.

Front 11

What specific types of molecules violate the Octet Rule?

Back 11

Any molecule with an overall odd # of electrons (ex. NO)

Front 12

When drawing Lewis Dot structures, which atom do you put in the center?

Back 12

The one that can make the most bonds.

Front 13

What is the Formal Charge and how do you calculate it?

Back 13

Its the charge on an individual atom in a molecule. Ideally, each atom in a Lewis Dot structure should be closest to 0. Formal Charge = Normal Valence Electrons - lines and dots

Front 14

Define the Hybridization, Bond Angle, EDG and MG when there are _2_ Electron Domains and _0_ Non-bonding Pairs of electrons.

Back 14

sp, 180, Linear, Linear (CO2)

Front 15

Define the Hybridization, Bond Angle EDG and MG when there are _3_ Electron Domains and _0_ Non-bonding Pairs of electrons.

Back 15

sp2, 120, trigonal planar, trigonal planar (BCl3)

Front 16

Define the Hybridization, Bond Angle EDG and MG when there are _3_ Electron Domains and _1_ Non-bonding Pairs of electrons.

Back 16

sp2, 119, trigonal planar, bent (SO2)

Front 17

Define the Hybridization, Bond Angle EDG and MG when there are _4_ Electron Domains and _0_ Non-bonding Pairs of electrons.

Back 17

sp3, 109.5, tetrahedral, tetrahedral (CH4)

Front 18

Define the Hybridization, Bond Angle EDG and MG when there are _4_ Electron Domains and _1_ Non-bonding Pairs of electrons.

Back 18

sp3, 107, tetrahedral, Trigonal pyramidal (NH3)

Front 19

Define the Hybridization, Bond Angle EDG and MG when there are _4_ Electron Domains and _2_ Non-bonding Pairs of electrons.

Back 19

sp3, 104.5, tetrahedral, bent (H2O)

Front 20

Define the Hybridization, Bond Angle EDG and MG when there are _5_ Electron Domains and _0_ Non-bonding Pairs of electrons.

Back 20

sp3d, 90/120/180, trigonal bipyramidal, trigonal bipyramidal (PCl5)

Front 21

Define the Hybridization, Bond Angle EDG and MG when there are _5_ Electron Domains and _1_ Non-bonding Pairs of electrons.

Back 21

sp3d, 101.5/173, trigonal bipyramidal, see-saw (SF4)

Front 22

Define the Hybridization, Bond Angle EDG and MG when there are _5_ Electron Domains and _2_ Non-bonding Pairs of electrons.

Back 22

sp3d, 87.5/<180, trigonal bipyramidal, T-shaped (ClF3)

Front 23

Define the Hybridization, Bond Angle EDG and MG when there are _5_ Electron Domains and _3_ Non-bonding Pairs of electrons.

Back 23

sp3d, 180, trigonal bipyramidal, linear (XeF2)

Front 24

Define the Hybridization, Bond Angle EDG and MG when there are _6_ Electron Domains and _0_ Non-bonding Pairs of electrons.

Back 24

sp3d2, 90/180, octahedral, octahedral (SF6)

Front 25

Define the Hybridization, Bond Angle EDG and MG when there are _6_ Electron Domains and _1_ Non-bonding Pairs of electrons.

Back 25

sp3d2, 85/180, octahedral, square pyramidal (BrF5)

Front 26

Define the Hybridization, Bond Angle EDG and MG when there are _6_ Electron Domains and _2_ Non-bonding Pairs of electrons.

Back 26

sp3d2, 90/180, octahedral, square planar (XeF4)

Front 27

Trigonal Bipyramidal has 2 positions for electron domains. What are they and which position do lone pairs prefer to be in?

Back 27

Axial (up and down) and Equitorial. LPs prefer to be in the Equitorial position.

Front 28

Do bonded electron pairs or lone pairs have a greater repulsion?

Back 28

LPs

Front 29

What type of orbitals can be used to make a sigma bond?

Back 29

s, p, or ANY hybrid orbital (sp, sp2, sp3, sp3d, etc.)

Front 30

What type of orbitals can be used to make a pi bond?

Back 30

ONLY p orbitals (sideways overlap)