Chemistry 8,9,10

Front 1

Trends in Atomic Radius

Back 1

As you go down and to the left the atomic radius gets bigger.
Largest radius is in bottom lefthand corner.

Front 2

Trends in effective nuclear charge (Zeff)

Back 2

as you move to the right, effective nuclear charge increases,

Front 3

paramagnetic

Back 3

When electrons are unpaired

Front 4

diamagnetic

Back 4

When electrons are paired.

Front 5

relationship between cations and atoms.

Back 5

cations (+) are much smaller than their respective atoms

Front 6

relationship between anions and atoms.

Back 6

anions (-) are significantly larger than their atom.

Front 7

Ionization Energy (IE)

Back 7

The energy needed to to remove an electron from the atom or ion in the gaseous state.

Front 8

Trends in First Ionization Energy

Back 8

As you move to the right and up the IE increases, making the uppper right hand corner the highest IE.

Front 9

Electron Affinity

Back 9

the energy change associated with the gaining of an electron by the atom in the gaseous state. Is usually negative because it is releasing energy when it gains an electron.
generally gets more negative and exothermic as you move to the right of the PT

Front 10

Metallic Character Trends

Back 10

As you move to the left and down the metallic character increases. Making the lower left hand corner the most mettalic.

Front 11

Hydridization for linear

Back 11

sp

Front 12

Hydridization for trigonal Planar

Back 12

sp 2

Front 13

Hydridization for tetrahedral

Back 13

sp 3

Front 14

Hydridization for trigoanl bipyramidal

Back 14

sp3d

Front 15

Hydridization for octahedral

Back 15

sp3d2

Front 16

Which hybridization has left over P orbitals?

Back 16

sp2

Front 17

Coulomb's law

Back 17

2 alike charged particles tend to repel , different charged particles attract

Front 18

Octet rule exceptions

Back 18

odd electrons
incomplete octets: Be and B
Expanded octets: Thirds period or below

Front 19

Shielding

Back 19

tendency for the core electrons to shield out electrons from nuclear charge

Front 20

Penetration

Back 20

Ability of electrons in outer orbitals to penetrate into the region occupied by core electrons-experiences full nuclear charge

Front 21

What electrons lose S electrons to make D electrons half fulled?

Back 21

Cr, Cu, Mo, Ag

Front 22

Are bonds breaking negative or positive?

Back 22

Positive-endothermic

Front 23

Are bonds forming negative or positive?

Back 23

Negative-exothermic

Front 24

2 e groups
2 bonding
0 lone pairs

Back 24

e-linear
m-linear

Front 25

3 e groups
3 bonding
0 lone pairs

Back 25

e-trigonal planar
m-trigonal planar

Front 26

3 e groups
2 bonding
1 lone pairs

Back 26

e-trigonal planar
m-bent

Front 27

4 e groups
4 bonding
0 lone pairs

Back 27

e-Tetrahedral
m-tetrahedral

Front 28

4 e groups
3 bonding
1 lone pairs

Back 28

e- tetrahedral
m-trigonal pyramidal

Front 29

4 e groups
2 bonding
2 lone pairs

Back 29

e- tetrahedral
m-bent

Front 30

5 e groups
5 bonding
0 lone pairs

Back 30

e- trigonal bipyramidal
m- trigonal bipyramidal

Front 31

5 e groups
4 bonding
1 lone pairs

Back 31

e-trigonal bipyramidal
m- seesaw

Front 32

5 e groups
3 bonding
2 lone pairs

Back 32

e- trigonal bipyramidal
m-t-shaped

Front 33

5 e groups
2 bonding
3 lone pairs

Back 33

e- trigonal bipyramidal
m-linear

Front 34

6 e groups
6 bonding
0 lone pairs

Back 34

e-octahedral
m-octahedral

Front 35

6 e groups
5 bonding
1 lone pairs

Back 35

e- octahedral
m-square pyramidal

Front 36

6 e groups
4 bonding
2 lone pairs

Back 36

e- octahedral
m- square planar