Electronic Structure of the Atom

Question 1

nodes

Answer 1

empty spaces between subshells

Question 2

S subshell

Answer 2

in all 7 pel, 1 orbital, max 2 electrons

Question 3

P subshell

Answer 3

2-7 pel, 3 orbitals, max 6 electrons

Question 4

d subshell

Answer 4

3-7 pel, 5 orbitals, max 10 electrons

Question 5

f subshell

Answer 5

3-5 pel, 7 orbitals, max 14 electrons

Question 6

S subshell shape

Answer 6

shperical

Question 7

p subshell shape

Answer 7

dumbbell

Question 8

d subshell shape

Answer 8

dumbbell and spherical

Question 9

f subshell

Answer 9

dumbbell and spherical

Question 10

electron configurations

Answer 10

short hand configurations used to indicate the location of electrons in an atom

Question 11

valence electrons

Answer 11

electrons found in the outer most principle energy level

Question 12

orbital energy diagrams

Answer 12

indicate the location of electrons as well as the energy of the electron

Question 13

hybridization

Answer 13

occurs when electrons shift to higher or lower orbitals

Question 14

elements that hybridize naturally

Answer 14

carbon, silicon, chromium, molybdenum, tungsten?

Question 15

Aufbau principle

Answer 15

electrons enter orbitals with the lowest energy first

Question 16

Pauli Exclusion Principle

Answer 16

no two electrons in any atom may have the same set of quantum numbers; therefore electrons within the same orbitals must have opposite spins

Question 17

Hund’s Rule

Answer 17

within a subshell; one electron will enter each orbital with parallel spins before pairing will begin

Question 18

electronegativity

Answer 18

the ability of an atom in a chemical compound to attract electrons

Question 19

Why does the electronegativity of an atom increase as you go up and across on the periodic table?

Answer 19

because as the number of protons increase down the group, the attractions decreases with distance

Question 20

electron shielding

Answer 20

when the valence electrons never feel the full force of the protons (attractive forces)

Question 21

ionization energy

Answer 21

the energy required to remove a valence electron

Question 22

What is the relationship between the atomic radius and the periodic table?

Answer 22

It increases as you go down and across from right to left.

Question 23

light

Answer 23

electromagnetic waves, which travel through a vacuum at a rate of 3.0x10^10 cm/sec

Question 24

How do you calculate frequency?

Answer 24

Frequency = # of waves (cycles) / second

Question 25

speed of light (C)

Answer 25

3.0 x 10^10 cm / sec

Question 26

blue shift

Answer 26

towards

Question 27

red shift

Answer 27

away

Question 28

line (discontinuous) spectra

Answer 28

when an element in its gas state exposed to an electric charge and the light emitted is passed through a prism

Question 29

quantum numbers

Answer 29

used to indicate the location of electrons in an atom

Question 30

ground state

Answer 30

when electrons are in the lowest possible energy levels

Question 31

n

Answer 31

pel

Question 32

l

Answer 32

subshell

Question 33

m1

Answer 33

orbital

Question 34

ms

Answer 34

e spin

Question 35

John Dalton

Answer 35

defined the atom as an indestructible mass

Question 36

Joseph Thomson

Answer 36

discovered the negatively charged electron, developed “Plum Pudding” model

Question 37

Ernest Rutherford

Answer 37

discovered nucleus with protons and neutrons, couldn’t explain why electrons didn’t collapse (they were quantized)

Question 38

Schrodiner

Answer 38

Schrodinger equation: describes mathematically the location and energy of electrons in the hydrogen atom