Atomic structure

Question 1

Mass Number

Answer 1

protons + neutrons

Question 2

Relative Atomic Mass

Answer 2

Average mass of all isotopes of an atom, relative to 1/12th of Carbon 12

Question 3

Isotopes

Answer 3

Different forms of the same element with same no. protons but varying no. Neutrons

Question 4

hydrogen emission spectrum

Answer 4

a series of discrete lines of light that converge at a higher frequency

Question 5

atomic number

Answer 5

no. protons in nucleus

Question 6

physical properties of isotopes

Answer 6

different due to differing masses

Question 7

chemical properties of isotopes

Answer 7

identical (same electron configuration/no. electrons in outer shell)

Question 8

radioisotope

Answer 8

atom with unstable nucleus which undergoes radioactive decay + emits a gamma ray and/or alpha/beta particle

Question 9

what are radioisotopes used for?

Answer 9

1. in nuclear medicine for diagnostics, treatment, research
2. as medical tracers in biochemical & pharmaceutical research
3. chemical clocks in geological & archaeological dating (radiocarbon dating)

Question 10

PET

Answer 10

positron emission tomography

Question 11

what do PET scanners do?

Answer 11

give 3D images of tracer concentration in the body + detect cancers

Question 12

process of PET scanners

Answer 12

1. radioactive tracer injected into bloodstream
2. tracer absorbed by active tissues of brain
3. PET scanner detects photons emitted by tracer
4. produce slice images

Question 13

electromagnetic spectrum

Answer 13

the distribution of electromagnetic radiation according to their energies

Question 14

white light is made of

Answer 14

all colors of spectrum

Question 15

when passed through a prism, white light is

Answer 15

split into a continuous spectrum containing all possible wavelengths/frequencies

Question 16

what happens when energy is supplied to a particular element?

Answer 16

it will emit a line spectrum

Question 17

when electrons are excited, they ___

Answer 17

move from lowest energy level (ground state) to a higher energy level

Question 18

what causes a line on the spectrum?

Answer 18

when an electron drops back into a lower shell, they emit energy of a specific wavelength

Question 19

amount of orbitals in sub-level

Answer 19

s=1 p=3 d=5 f=7

Question 20

electron orbital

Answer 20

the region/volume where an electron is most likely to be

Question 21

electrons are arranged in ___

Answer 21

electron shells (energy levels)

Question 22

4 types of sub-shells

Answer 22

spdf

Question 23

each sub-shell is made up of __ __ , which can each hold __ electrons (__ principle)

Answer 23

electron orbitals, 2, Heisenberg

Question 24

each electron orbital can contain a maximum of __ electrons spinning in __ directions (__ __ Principle)

Answer 24

2, opposite, Pauli Exclusion

Question 25

each sub-shell has orbitals of __ __

Answer 25

different shape

Question 26

aufbau principle

Answer 26

electrons must be put in orbitals of lowest energy first

Question 27

hund's rule

Answer 27

when filling sub-shells, each orbital must contain **1 electron before pairing up**

Question 28

4s subshell must be filled __ the 3d subshell

Answer 28

before

Question 29

what happens when 4s and 3d are occupied?

Answer 29

4s moves above 3d

Question 30

isoelectronic

Answer 30

same electronic configuration

Question 31

Exceptions

Answer 31

Cr (4s1 3d5) Cu (4s1 3d10)

Question 32

example of radioisotopes used in medicine

Answer 32

Tc-99m: diagnostic imaging in brain, heart, bone, kidney scans

Question 33

Relative mass of electrons

Answer 33

5x10^4

Question 34

Position of electrons

Answer 34

Energy levels

Question 35

Number of orbitals present

Answer 35

n^2

Question 36

Max electron occupancy

Answer 36

2n^2

Question 37

ER Longest to shortest wavelength

Answer 37

RMIVUXG Radio, microwaves, infrared, visible light, UV, X-rays, gamma rays

Question 38

Valence electrons define the __ of the element

Answer 38

Group number

Question 39

Frequency is directly proportional to

Answer 39

1/wavelength

Question 40

n=1 contains _ orbitals (_ total)

Answer 40

S, 1

Question 41

n=2 contains _ orbitals (_ total)

Answer 41

s, px, py, pz, 4

Question 42

n=3 contains _ orbitals (_ total)

Answer 42

s, px, py, pz, d(5), 9

Question 43

1s2 what does each represent

Answer 43

1=principal energy level, s=subshell 2=no. electrons

Question 44

n=4 contains _ orbitals (_ total)

Answer 44

s, p(3), d(5), f(7)

Question 45

alpha particle charge

Answer 45

positive

Question 46

n=1 light emitted

Answer 46

UV (Lyman)

Question 47

n=2 light emitted

Answer 47

visible (Balmer)

Question 48

n=3 light emitted

Answer 48

IR (Paschen)

Question 49

bohr's hydrogen atom

Answer 49

electron moving in an orbit/energy level around the positively charged nucleus of **1 proton**

Question 50

The electrostatic force between electrons and protons does what?

Answer 50

prevents electrons from **leaving** the atom

Question 51

Without the neutrons, what happens?

Answer 51

protons mutually repel each other + the nucleus falls apart

Question 52

rutherford's findings

Answer 52

atom is mostly empty space + posititvely charged nucleus

Question 53

rutherford's gold foil

Answer 53

most alpha particles passed through (empty space), some deflected (nucleus)

Question 54

Sub-shell

Answer 54

Subdivision of electron shells

Question 55

Electron shell

Answer 55

Energy level within an atom

Question 56

Longest to shortest wavelength colors

Answer 56

Red, orange, yellow, green, blue, indigo, violet