Unit 6: Electron Structure in Atoms

Question 1

True or false.

light is a wave

Answer 1

TRUE

Question 2

Definition of electromagnetic radiation

Answer 2

carries energy through space

• creates electromagnetic fields
• creates the electromagnetic spectrum

Question 3

What is the equation to find either wavelength or frequency?

Answer 3

c = λ * V
v=frequency
λ= wavelength
C= speed of light 3.0 x 10^8 m/s

Question 4

Definition of wavelength

Answer 4

The distance between two points (crest or trough) on a wave

Question 5

Definition of amplitude

Answer 5

The distance from a crest or trough to the middle line

Question 6

Definition of frequency

Answer 6

The number of cycles that pass a point per second

Question 7

How is frequency measure?

Answer 7

measured in cycles/second or S-1 or Hertz (Hz)

Question 8

Horizontal rows on the periodic table are….?

Answer 8

periods

Question 9

What does the periods mean?

Answer 9

n= outermost energy level that is occupied with electrons

Question 10

Definition of black-body radiation

Answer 10

The emission of light from hot substances

• The wavelength of light depends on the temp
• red hot substances are cooler than white hot substances

Question 11

Who is Max Planck?

Answer 11

• German physicist
• assumed that energy can be released by atoms only in discrete “chunks” of some minimum size.
• atoms cant cont. emit or absorb energy
• BUNDLES OF ENERGY

Question 12

Definition of quantum

Answer 12

The smallest quantity of energy that can be emitted or absorbed as electromagnetic radiation

Question 13

What is the equation to find the energy of a single quantum? E=….

Answer 13

E = hv
h= planck's constant 
v= frequency

Question 14

What is planck’s constant?

Answer 14

6.63X10^-34 J*s

Question 15

What is planck’s quantum theory?

Answer 15

energy is always emitted or absorbed in whole number multiples of hv

Question 16

What is photon emission?

Answer 16

This is when light is given off and and electron falls down to a lower energy level

Question 17

What is photo absorption?

Answer 17

This is when light hits an atom and makes an electron jump to a higher energy level

Question 18

What is the photoelectric effect?

Answer 18

Light of a certain frequency causes atoms on the surface to emit electrons

Question 19

What did albert einstein come to the conclusion when he put together planck and applied it to the photoelectric effect?

Answer 19

Energy hitting the metal is a stream of tiny energy packets

• energy of photon is proportional to the frequency
• E (energy of photon) = hv

Question 20

Fill in
____ light frequency= _____ energy photons = ____ to eject electrons

____ light intensity = ____ electrons ejected from atoms

____ light frequency (v) = ____ speed of electrons ejected from atoms

Answer 20

1. Higher, higher, easier
2. higher, more,
3. Higher, faster

Question 21

Definition of spectrum?

Answer 21

produced when radiation of various wavelengths is separated (light bulbs, stars)

Question 22

Definition of continuous spectrum?

Answer 22

contains all wavelengths of light (rainbow)

Question 23

Definition of monochromatic?

Answer 23

having only one wavelength of light (laser)

Question 24

Definition of line spectrum?

Answer 24

a spectrum containing radiation only of certain wavelengths

Question 25

What are Bohr's 2 major ideas?

Answer 25

1. electrons exist only in discrete energy levels; quantum numbers 2. energy is involved in moving an electron from one level to the next

Question 26

What did Louis de Broglie think of?

Answer 26

an electron behaves like a wave as it moves around the nucleus and has a specific wavelength - Matter Wave *the λ of the electron depends on its mass and velocity (called momentum)

Question 27

What is an equation to find λ?

Answer 27

λ = h / mv h=planck's constant m=mass v=velocity

Question 28

What is the Heisenberg uncertainty principle?

Answer 28

impossible to know exactly where an electron is around the atom

Question 29

What did Erwin Shrodinger come up with?

Answer 29

Developed the wave equation proposal * developed wave functions that describe the electrons matter wave * the location of electrons is based on these and probability

Question 30

What do orbitals look like and what three ideas go wiith them?

Answer 30

look like clouds * have diff shapes * have diff energies * orbitals are diff than orbits (which are simple circles)

Question 31

What are the 3 quantum #'s in the quantum mechanical model?

Answer 31

1. principal quantum number 2. azimuthal quantum number 3. magnetic quantum number

Question 32

What is the principal quantum number?

Answer 32

n=1, 2, 3, etc * gives the level of the orbital * as n increases the orbital becomes larger * as n increases the electron has more energy and is less tightly bound to the nucleus * shell=orbit=energy level

Question 33

What is the azimuthal quantum number?

Answer 33

ℓ = 0 to n-1 *defines shape s, p, d, f *orbital=subshell ℓ = 0, orbital letter s, shape= spherical ℓ = 1, orbital letter p, shape principal (infinity sign) ℓ = 2, orbital letter d, shape diffuse (four leaf clover) ℓ = 3, orbital letter f, shape fundamental (crazy shape dont need to know)

Question 34

What is the magnetic quantum number?

Answer 34

mℓ = symbol * values of ℓ to -ℓ (including 0) * defines the orientation in space (x,y,z)

Question 35

What do the 3 numbers for the quantum mechanical model?

Answer 35

probable location of an electron

Question 36

What is the 4th quantum number?

Answer 36

Ms = the spin magnetic quantum number * indicates what direction the electron spins * 2 values +1/2 or -1/2

Question 37

Definition of Aufbau principle?

Answer 37

electrons enter orbitals with the lowest energy first. this means that electrons must fill the first energy first level before placing any in the second

Question 38

Definition of Pauli exclusion principle?

Answer 38

each atomic orbital contains a maximum of two electrons.

Question 39

Definition of Hund's Rule

Answer 39

Electrons enter each orbital of a given type singly and with identical spins before any pairing of electrons of opposite spin occurs within those orbitals *each orbital of a certain shape receives one electron before you can double them up

Question 40

What is the diff between electron configuration and orbital diagram?

Answer 40

the diagram has the arrows and the configuration is just numbers ans letters (ex. 1s^2 2s^2....)