Chapter 1- Atomic Structure

Question 1

(Z)

Answer 1

Atomic number. Different for each elements. Tells the amount of protons in an element

Question 2

(A)

Answer 2

Atomic number. Tells the number of protons and neutrons in the nucleus of an elements.

Question 3

Isotope, What subatomic particle differs between isotopes?

Answer 3

Atoms that share an atomic number (Z) but have different mass numbers (A)

Different number of neutrons.

Question 4

Fundamental unit of charge

Answer 4

e= 1.6x10^-19

Proton + 1.6x10^-19
Electron - 1.6x10^-19

Question 5

Between electrons and protons which is larger?

Answer 5

Protons.

Electrons are approximately 1/2000 the size of a proton

Question 6

Electrons closer to the nucleus have higher low energy levels. Electrons further away from the nucleus have higher low energy levels

Answer 6

Electrons closest to the nucleus have low energy levels while electrons further away from the nucleus have high energy levels which is why they are the electrons that interact with other molecules.

Higher energy level equals less negative

Question 7

Cation vs Anion

Answer 7

Cation: positively charged atom
Anion: negatively charged atom

Question 8

Atomic weight vs Atomic mass

Answer 8

Atomic mass is nearly equal to an atoms mass number, the sum of protons and neutrons.

Atomic weights is the weighted average of all of an atoms different isotopes.

Question 9

Avogadro’s number

Answer 9

6.02×10^23

A mole is equal to Avogadro’s number 

Question 10

Planck’s equation

Answer 10

E=hf

E=energy of a quantum (Energy emitted from matter comes in discrete bundles called quanta) 
Planck’s constant (h) 6.26×10^-34 J x s
f= frequency of radiation

Question 11

Planck’s constant

Answer 11

(h)

6.26×10^-34

Question 12

E

Answer 12

E=energy of a quantum

Energy emitted from matter comes in discrete bundles called quanta

Question 13

Speed of light

Answer 13

C is equal to 3×10^8m/s

Question 14

What equation do you use to calculate the angular momentum of an electron orbiting a hydrogen nucleus?

Answer 14

L=nh/2pi

Question 15

L=nh/2pi

Answer 15

Equation that tells the angular momentum of an electron orbiting the nucleus

L:angular momentum

n: principal quantum number
h: planck’s constant

Question 16

How to calculate the energy of the electron?

Answer 16

E=-Rh/n^2

E: Energy of the electron
Rh: Rydberg unit of energy (experimentally determined) 2.18-10^-18 J/electron
n: distance from nucleas (bigger the n the greater the energy, less negative)

Question 17

Ground state versus excited state

Answer 17

Ground state is the state of lowest energy (smaller in value) excited state is when one electron is moved to a sub shell of higher than normal energy.

Question 18

From a lower energy level to a higher energy level they get…

Answer 18

AHED

A- Absorb light
H-Higher potential
E-Excited
D-distance (from the nucleus)



Question 19

How do you determine the electromagnetic energy of a photon?

Answer 19

E=hc/lambda

Electromagnetic energy
H=planck’s constant
C=speed of light (3x10^8m/s)
Lambda=Wavelength of the radiation

Question 20

When an electron returns back to ground state does is energy absorbed or omitted?

Answer 20

Energy is emitted through a photon

Question 21

How do you calculate the energy of the emitted photon when it moves from a higher initial states to a lower initial state?

Answer 21

E=hc/lambda= -Rh[1/ni^2-1/nf^2]

Rh: Rydberg unit of energy (2.18×10^-18 J/electron)

Question 22

Moving from high to low energy levels versus moving from low to high energy levels

Answer 22

Moving from high to low energy levels energy is emitted (emission). Moving from low to high energy levels energy is absorbed (absorption) 

Question 23

n

Answer 23

Principal quantum number.

Gives you the shell an electron resides in.

Possible values include nonzero integers

Question 24

l

Answer 24

Azimuthal (angular momentum) quantum number

Tells you the shape and number of subshells

Possible values include 0 to n-1 

Question 25

ml

Answer 25

Magnetic quantum number

Tells you the particular orbital within a subshell where an electron is most likely to be found at a given moment of time.

Possible values between -l and +l

Question 26

Maximum number of electrons per orbital

Answer 26

2

Question 27

Which blocks of the periodic table do the following azimuthal numbers correlate with: I=0, I=1, I=2, l=3.

Answer 27

I=0 s
I=1 p
I=2 d
l=3 f

Question 28

How do you figure out the maximum number of electrons within a sub shell?

Answer 28

4l +2

Question 29

Shape of s orbital vs p orbital

Answer 29

Orbitals in the s subshell are spherical, the three orbitals of the p subshell are dumbbell shaped and aligned along the XY and Z axis

Question 30

ms

Answer 30

Spin quantum number

Possible orientations include +1/2 and -1/2

Question 31

n+1 rule

Answer 31

A rule that shows you which subshell should be filled first. The lower the sum of n+l the lower the energy of the subshell.

If two subshells possess the same n+1 value the subshell with the lower n value will fill first.

Or you can just read the periodic table 😜

Question 32

How do you find the electron configuration of an ion?

Answer 32

For a cation electrons are removed from the highest sub shell

For an anion electrons are added to the highest subshell

Question 33

Elements in which period and below accepts electrons into their d subshell which allows them to violate the octet rule

Answer 33

Period 3

Question 34

Hunds rule

Answer 34

Within a given sub shell orbitals are filled such that there are a maximum number of half filled orbitals with parallel spins. Electrons would prefer to have their own are available for being forced to double up with another electron.

Half filled and fully filled orbitals have a lower energy than other states.

Question 35

Which elements and their groups are the exceptions to electron configuration?

Answer 35

Chromium (4s1 3d5) and Copper (4s1 3d10)

One electron is moved from the 4s sub shell to the 3d sub shell to allow the 3d subshell to be half filled

Question 36

Paramagnetic

Answer 36

Material composed of atoms with unpaired electrons orient their spins in alignment with the magnetic field. The material willl thus be weakly attracted to the magnetic field.

Paramagnetic means the magnetic field will cause parallels in unpaired electron therefore causing attraction. 

Question 37

Diamagnetic

Answer 37

Materials with items that only have paired electrons will be slightly repelled by a magnetic field.

Question 38

When drawing an orbital diagram how many orbitals are in the s,p,d subshells?

Answer 38

S=1
P=3
D=5

Question 39

Heisenberg uncertainty principle

Answer 39

Position and velocity are related and cannot be simultaneously determined

Question 40

Hunds Rule

Answer 40

Electrons in a subshell will only pair when the orbital is half filled

Question 41

Aufbau’s principle

Answer 41

Electrons will fill lower energy orbitals before filling higher energy orbitals

Question 42

Pauli’s exclusion principle

Answer 42

No two electrons in an atom can have the same exact quantum numbers