Chemistry Unit 2 And A Half?

Front 1

What happens when two atoms in a linear model have equal and opposite electro negativities?

Back 1

They cancel and are non-polar.

Front 2

What happens when you have more than one bond in a molecule?

Back 2

Determine if the are polar or non polar because they have dipoles! Use the VSEPR theory.

Front 3

What happens if the end atoms in a linear model are unequal?

Back 3

It's Polar!

Front 4

What is a bent molecule with all three elements having the same electro negativities?

Back 4

Its nonpolar!

Front 5

What is a bent molecule with different electronegativities?

Back 5

polar!

Front 6

What is a pyramidal molecule with all the same electronegativities?

Back 6

non polar!

Front 7

What is a pryamidal molecule with different electronegativities?

Back 7

polar!

Front 8

If all 4 atoms that surround the central atom of a tetrahedral have the same electro negativity, what is it?

Back 8

nonpolar!

Front 9

How many bonding groups and lone pairs do a linear shape have?

Back 9

2 bonding groups and 0 lone pairs.

Front 10

How many bonding groups and lone pairs do a trigonal planar have?

Back 10

3 bonding groups and 0 lone pairs

Front 11

How many bonding groups and lone pairs do a tetrahedral shape have?

Back 11

4 bonding groups and 0 lone pairs.

Front 12

How many bonding groups and lone pairs do a pyramidal shape have?

Back 12

3 bonding groups and 1 lone pair.

Front 13

How many bonding groups and lone pairs do a bent shape have

Back 13

2 bonding groups and 2 lone pairs.

Front 14

Name the structure and properties of ionic compounds?

Back 14

They are hard crystalline solids with high melting and boiling points. They are brittle and and break easily when bent. They conduct ionic compounds conduct electricity in the molten state or if dissolved in water to form an aqueous solution.

Front 15

Explain why Ionic compounds are hard crystalline solids with high melting and boiling points?

Back 15

They have stable structures. Cations are surrounded by anions and anions are surrounded by cations.
A considerable amount of heat must be applied to an ionic compound to get its particles moving fast enough to overcome forces of attraction.

Front 16

Explain why Ionic compounds are brittle and break easily.

Back 16

If force is applied to an ionic compound by bending or hitting, the cations and anions may be shifted towards ions with the same charge as themselves. This results in repulsions between the ions and since the stable crystal lattice is disrupted, the compound shatters.

Front 17

Why do ionic compounds conduct electricity when in a molten aqueous state?

Back 17

The electrons can move freely throughout the compound. This flow is called electricity! Therefore melting and dissociation allows an ionic compound to become conductive.

Front 18

What are the structures and properties of molecular compounds?

Back 18

Molecular compounds share electrons to become stable, They also generally have lower melting and boiling points than ionic compounds.

Front 19

What are the three types of molecular substances?

Back 19

Molecular elements, Compounds and network solids.

Front 20

Molecular Elements

Back 20

these are diatomic and cyclic. They have the lowest melting/boiling points of all molecular compounds.

Front 21

Molecular Compounds

Back 21

Have two or more elements bonded together. They have a wide range of melting/boiling points that are higher than that of a element but lower than ionic compounds.

Front 22

Network Solids

Back 22

3-D network of nonmetallic atoms held very tightly together to form single large molecules. They are very stable and are extremely hard and have unusually high melting/boiling points.

Front 23

What are the structures and properties of metallic bonding?

Back 23

Metals are malleable. They are good conductors. They have a wide range of melting and boiling points. Metals form alloys.

Front 24

What are Intra-molecular forces?

Back 24

Forces that keep the atoms in a compound stuck to each other. They're just chemical bonds.

Front 25

What are Intermolecular forces?

Back 25

The forces that attract two covalent molecules to one another. Intermolecular forces are found ONLY IN MOLECULAR COMPOUNDS.

Front 26

What are the 3 main types of intermolecular forces?

Back 26

London Dispersion Forces, Dipole-Dipole Forces, and Hydrogen Bonding.

Front 27

What are London Dispersions Forces?

Back 27

Referred to as LDF. LDF forces occur when nonpolar molecules stick together due to magnectic attractions. LDF are the weakest of all 3 intermolecular forces.

Front 28

How do we determine how strong LDF's are in a compound?

Back 28

1. All molecular compounds have LDF.
2. The strength of LDF depends on the number of electrons present in a molecule (determined from atoms atomic number.) and he molecules shape or complexity. The stronger the LDFs, the stronger the forces of attraction and highter the melting/boiling point.

Front 29

What are Dipole-Dipole forces?

Back 29

Forces found between polar molecules. They are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.

Front 30

What is hydrogen bonding?

Back 30

Hydrogen bonds are found in polar molecules. The molecules that undergo hydrogen bonding all contains a hydrogen atom that is bonded to a nitrogen, oxygen, or fluorine.

Front 31

What order has the highest to lowest boiling points?

Back 31

1. Network solids
2. Ionic compounds
3. Molecular compounds that go in the order of i) LDF ii) Dipole-Dipole iii) Hydrogen bonding