Chemistry - Final (Unit 3)

Front 1

how many electrons can hydrogen and helium hold?

Back 1

2

Front 2

metals tend to ___ their electrons while nonmetals tend to ___

Back 2

lose, gain, because metals have fewer valence electrons

Front 3

ionic bonds tend to have ___ melting and boiling points and are found as ___ at room temp

Back 3

high, solids

Front 4

Polar covalent bonds have the ____ melting and boiling points and are mostly ____ or ___ at room temp

Back 4

next to highest, solids or liquids

Front 5

Non-polar covalent bonds have ____ melting and boiling points and are mostly found as ___ or ____

Back 5

lower, liquids or gases

Front 6

ionic and polar covalent compounds tend to be ___ in water

Back 6

soluble

Front 7

Nonpolar and metallic compounds tend to be ____

Back 7

insoluble

Front 8

In order to conduct electricity a charge must be able to ____

Back 8

move/flow

Front 9

___ bonds have free-moving electrons, they can conduct electricity in a solid and liquid state

Back 9

metallic

Front 10

___ bonds have free-floating ions when dissolved in water or liquid form allow them to conduct electricity

Back 10

ionic

Front 11

___ bonds never have charges free to move and can't conduct electricity

Back 11

covalent

Front 12

polarity of molecules# An attraction an atom has for a shared pair of electrons is called ____

Back 12

Electronegativity

Front 13

Higher EN in an atoms has a ____ charge

Back 13

partially negative

Front 14

The lower Electronegativity atom has a ____ charge

Back 14

partially positive

Front 15

Electronegativity ____ up and to the right

Back 15

increases

Front 16

the difference in electronegativity between the atoms in a chemical bond determines the ___

Back 16

bond type

Front 17

the difference in electronegativities of two atoms involved in a bond is less than or equal to 4.0, then they are considered to be pulling electrons in similar amounds that the bond is ____

Back 17

nonpolar covalent

Front 18

If the electronegativity difference is greater than 4.0 and less than 2.0, then the bond is ___

Back 18

polar covalent (not sharing the bonding pair evenly)

Front 19

If the EN difference is above 2.0 then the bond is an ____

Back 19

ionic bond, (as occurs when a metal and a nonmetal bond) the difference is so great that they don't share at all, one atom takes the electrons from the other atom

Front 20

-electrons are shared equally
-symmetrical
-usually identical atoms

this describes what type of bond

Back 20

nonpolar covalent

Front 21

-electrons are shared unequally
-asymmetrical
-results in partial charges (dipole)

Back 21

polar covalent bond (partially neg on one end, partially pos on other end)

Front 22

arrow points toward the more electronegative atom

Back 22

ok

Front 23

to determine ____ bonds the shape is symmetrical and the charges cancel out (draw line, both ends positve or neg.)

Back 23

nonpolar covalent

Front 24

to determine ____ bonds the shape is asymmetrical and the charges don't cancel out (pos on one side, neg on another)

Back 24

polar molecules

Front 25

forces within the molecule (chemical bonds) are called ____ forces

Back 25

intramolecular

Front 26

Forces between separate molecules are called ____ forces

Back 26

intermolecular (IMF)

Front 27

IMF (forces between molecules) are much ___ than intramolecular forces (forces within molecule)

Back 27

weaker

Front 28

_____ are attractions between temporarily polar molecules. it's an intermolecular force (a weak one) because it's temporary
-the strength of this forces is greater as the number of electrons in a molecule increases

Back 28

london dispersion forces (LDF)

Front 29

which molecules have london dispersion forces?

Back 29

all molecules

Front 30

similiar polar intramolecular force to London dispersion forces except it's permanent ___

Back 30

dipole dipole

Front 31

The interaction between polar molecules that are also intermolecular forces are called _____

Back 31

dipole dipole

Front 32

where does dipole dipole occur?

Back 32

in all polar molecules.

Front 33

which is stronger, dipole dipole or LDF?

Back 33

dipole dipole because the molecules always have the capability of forming them with other polar molecules

Front 34

this describes what force, -the bond is not a full covalent bond, it is not an intramolecular force but is a strong attraction between a hydrogen atom on one molecule and an electronegative element on another molecule

Back 34

Hydrogen bonding

Front 35

______ is the strongest of the types of intermolecular forces

Back 35

hydrogen bonding

Front 36

_____ bonding is a specific, strong case of Dipole diople interaction. the reason that the bond is so strong is that when another electronegative element shares unevenly with hydrogen, hydrogen has no other electrons around its nucleus to counteract the positive charge of the nucleus.

Back 36

hydrogen

Front 37

breaking of intermolecular forces (between separate molecules) is a ___ change

Back 37

physical (breaking glass, boiling water)

Front 38

larger molecules and molecules with high IMFs have more ____

Back 38

viscocity

Front 39

the stronger the IMFs are, the _____ the melting and boiling points are

Back 39

higher

Front 40

water needs more energy to break apart it's IMF which is why water and oil don't mix. water can only form LDF with oil

Back 40

ok

Front 41

Soap has a ____ head with a ____ tail

Back 41

polar, nonpolar

Front 42

the ___ portion of soap can interact with water(polar) and the non polar portion can interact with dirt and grease (nonpolar)

Back 42

polar

Front 43

soap ____ the surface tension in water

Back 43

lowers

Front 44

a compound does not dissolve in water what type of bond?

Back 44

polar

Front 45

a compound dissolves in water but does not conduct electricity what type of compound?

Back 45

nonpolar

Front 46

a compound dissolves in water and conducts electricity when dissolved, what type of compound?

Back 46

ionic

Front 47

hydrogen bonds happen between which three elements

Back 47

H-O H-C H-F

Front 48

dipole dipole only happens in what molecules?

Back 48

polar