Chemistry Chapter 1

Question 1

Atomic number meaning

Answer 1

Number of protons

Question 2

Mass number meaning

Answer 2

Number of protons plus neutrons

Question 3

Electrons how you calculate

Answer 3

Basically same as protons unless there charge

Question 4

No isotopes has an exact equal to elements atomic weight < T or F

Answer 4

True
It is approximate of their two most commonly found isotopes

Question 5

Atomic weight meaning

Answer 5

The weight average of the commonly found isotopes of an element

Question 6

Is atomic mass the same as mass number

Answer 6

Yes basically the same

Question 7

Avogrados number

How many mols is that

Let’s say for example for carbon, what does that mean if its 12g

Answer 7

6.02 x 10^23

1 mol of an element is this much

It means that 6.02 x 10^23 carbon atoms have a combined mass of 12.0 grams. ( atomic weight )

Question 8

Planck constant is

Answer 8

6.626 x 10^-34 J x s

Question 9

What is the Planck relation equation
What is it trying to find

Answer 9

E=hf

Energy of a quantum

Question 10

Angular momentum of an electron equation

Answer 10

L= nh/2pi

Question 11

Energy of electron

Answer 11

E =2.718 - (R)/n^2

Question 12

Rydberg unit of energy is

Answer 12

2.18 x 10^-18

Question 13

Is energy directly proportional to quantum number

Answer 13

Yes

Question 14

When electrons go from low to high energy level they get AHED, what that mean

Answer 14

Absorb light
Higher potential
Excited
Distant from nucleus

Question 15

When electrons move to valence does energy increase or decrease
Also what is emitted with energy

Answer 15

Increase
Photon

Question 16

Electromagnetic energy of photons equation

Answer 16

E =hc/wavelength

Question 17

What is

Lyman series
Balmer series
Paschen series

Which has the largest wave transition

Answer 17

N > 2 to n=1

N>3 to n=2

N>4 to n=3

Lyman

Question 18

The energy of the emitted photons correspionds to the difference in energy between what

Answer 18

High energy initial state and lower energy final state

Question 19

Is energy proportional or inversely proportional to wavelength

Answer 19

Inversely

Question 20

What priceipal tells us we can’t locate an electrons exact positionc

Answer 20

Heisenbergnberg uncertainty principle

Question 21

What are the quantum numbers, from vague to detailed

Answer 21

N

l

ml

Ms

Question 22

The larger the principally quantum numbers (n) , what differencene does it make to RAdius and energy elvels

Answer 22

the higher the energy level and RAdius of the electron’s shell

Question 23

Photon calculations can be done which formula

Answer 23

E=hc/wavelength

Question 24

What is Lyman series
What is balmer series
What is paschen series

Most energy in

Answer 24

N>2 to n=1

N>3 to n=2

N>4 to n=3

Lyman

Question 25

What principal tells us we can’t catch exact moment of electron

Answer 25

Heisenberg uncertainty principal

Question 26

Quantum numbers from vague to detailed

Answer 26

N l ml ms

Question 27

What does a larger primary quantum number (n) indicate

Answer 27

Higher energy level and bigger radius of electron shell

Question 28

How to calculate principal quantum numbers energy difference Let’s say n=3 and n=4 shell difference

Answer 28

1/(3^2) - 1/(4^2)

Question 29

For any value of principal quantum numbers, there will be possible values for l ranging from what to what

Answer 29

0 to n-1

Question 30

What does l quantum numbers refer to

Answer 30

Shape and number of subshell

Question 31

L=0 L=1 L=2 L=3 Subshells are notated as

Answer 31

Spdf

Question 32

If n=4 and l=2 then what notation does this have

Answer 32

4d

Question 33

What is the maximum number of electrons within a subshell

Answer 33

4l+2

Question 34

Third quantum number specifies what

Answer 34

Particular orbital within subehll where electron is most likely to be found

Question 35

For any value of l, what are the possible values of ml

Answer 35

2l+1

Question 36

For any n. How many orbital

Answer 36

N^2

Question 37

For l =0 L=1 L=2 what are the possible ml values

Answer 37

L=0 limits ml to 0 (1) L=1 limits ml to -1,0,1 (3) L=2 limits ml to -2 to 0 to 2 (5)

Question 38

What does spin quantum numbers (ms) tell us about

Answer 38

Spin orientation of positive or negative 1/2

Question 39

Two electrons in teh same orbital must have what type of spins

Answer 39

Opposite

Question 40

What does the n+l rule tell us

Answer 40

The smaller the sum of primary and secondary quantum numbers, the lower the energy of the subshell

Question 41

Will 5d or 6s subshell fill first and why explain

Answer 41

6s Because 5d is n=5 and l=2, so 7 And 6s is n=6 and l=0 so 6 Since 6s is smaller value it fills first

Question 42

When you do electron configuration, d and f are always how many rows behind what it is shown on periodic table

Answer 42

D is always one row behind F is always 2 rows behind

Question 43

When you have an element that has a charge, how do you know where to minus or increase the electrons from

Answer 43

The one with the highest primary quantum numbers, so starting number

Question 44

According to hounds rule how would you fill shells

Answer 44

Half full first

Question 45

What are the 2 exceptions to hunds rule , which 2 elements What happens in those

Answer 45

Chromium And copper Th electron in the s subshell gets moved to d for increased stability

Question 46

Paramagnetic means that a magnetic field will cause what type of spins in unpaired electron And what does it cause

Answer 46

Parallel spins Attraction

Question 47

Repelling electrons in the magentic sense are called

Answer 47

Diamagnetic

Question 48

How do you what are the valence electrons of an element for each subshell

Answer 48

S is only s P is s and p D is s and d F is s and f

Question 49

Vanadium which electrons are valence and how many

Answer 49

5 valence electrons 2 in 4s and 3 in 3d

Question 50

Atoms with unpaired electrons on magnetic field are para or diamagnetic

Answer 50

Paramagnetic

Question 51

Speed of light

Answer 51

3 x 10^8 Q