Atomic Orbitals, Electronic Configurations and the Periodic Table

Question 1

what are regions of high probability of finding a electron called?

Answer 1

Atomic Orbitals

Question 2

what are the four orbital shapes?

Answer 2

s,p,d,f

Question 3

why is the s orbital in the first shell smaller than that of the s orbital in the second shell?

Answer 3

their diameter increases as the shell number increases

Question 4

how many electrons can each s orbital hold?

Answer 4

can only hold two electrons of opposite spins

Question 5

what term can be used to describe p orbitals?

Answer 5

degenerate

Question 6

what does the term degenerate mean?

Answer 6

orbitals of equal energy

Question 7

principal quantum number (n):

Answer 7

this number indicates the electrons main energy level

Question 8

angular momentum quantum number (l):

Answer 8

determines the shape of the orbital
(n-1)

Question 9

magnetic quantum number (ml):

Answer 9

determines the orientation of the orbital
values between -l and +l

Question 10

spin magnetic quantum number (ms):

Answer 10

indicates the direction in which the electron is spinning.
Either clockwise or anti-clockwise (-1/2, +1/2)

Question 11

Pauli Exclusion Principle:

Answer 11

“no two electrons in the same atom can have the same four quantum numbers, so no orbital can contain more than two electrons, and the two electrons must have opposite spins”

think can’t live at same address, Pauli/Paula

Question 12

Aufbau Principle:

Answer 12

“electrons fill the subshells in order of increasing energy”

Question 13

Hund’s Rule:

Answer 13

“when the degenerate orbitals are available, electrons fill each degenerate orbital singly and with parallel spins, before pairing to fill the orbitals”

Question 14

what is the rule with the electronic configuration of atoms to ions?

Answer 14

atoms form ions which have the electronic configuration of the nearest noble gas

Question 15

what is meant by the term isoelectronic?

Answer 15

particles which have the same electronic configuration

Question 16

what is meant by the ground state?

Answer 16

when the electrons are in their lowest possible energy level

Question 17

how are covalent bonds formed?

Answer 17

when two atomic orbitals combine to form a molecular orbital

Question 18

how do atomic orbitals combine to forma molecular orbital?

Answer 18

usually, both orbitals are half-filled and overlap to form a molecular orbital

Question 19

when is a dative covalent bond formed?

Answer 19

when one atom provides both the electrons that form the bond

Question 20

what formula can be used to calculate the number of electron pairs?

Answer 20

electrons of central atom+atoms attached/2

Question 21

what is the shape/bond angle of a molecule with two bonding pairs?

Answer 21

linear shape
180°

Question 22

what is the shape/bond angle of a molecule with three bonding pairs?

Answer 22

trigonal planar shape
120°

Question 23

what is the shape/bond angle of a molecule with four bonding pairs?

Answer 23

tetrahedral
109.5°

Question 24

what is the shape/bond angles of a molecule with five bonding pairs?

Answer 24

trigonal bipyramidal
120° and 90°

Question 25

what is the shape/bond angle of a molecule with six bonding pairs?

Answer 25

octahedral
90°

Question 26

what is the shape/bond angle of a molecule with two bonding pairs and one lone pair?

Answer 26

angular
120°

Question 27

what is the shape/bond angle of a molecule with three bonding pairs and one lone pair?

Answer 27

trigonal pyramidal
107.5°

Question 28

what is the shape/bond angle of a molecule with two bonding pairs and two lone pairs?

Answer 28

angular
104.5°

Question 29

what is the shape/bond angles of a molecule with three bonding pairs and two lone pairs?

Answer 29

t-shaped
120° and 86°

Question 30

what is the shape/bond angle of a molecule with four bonding pairs and two lone pairs?

Answer 30

square planar
90°