Nuclear Chemistry

Front 1

A ______ is a particle that is composed of 2 or more atoms held together by a chemical bond

Back 1

molecule

Front 2

______ are atoms of an element with identical chemical properties, but different masses due to a difference in the # of neutrons.

Back 2

Isotopes

Front 3

The _______ of an element is the avg. of all the atomic masses of the isotopes

Back 3

Atomic mass

Front 4

An isotope contribution is determined by its _______

Back 4

relative abundance

Front 5

________ is the mass of nucleus

_______ + _______

Back 5

atomic mass

protons + neutrons

Front 6

The __________ is also equal to the # of electrons and # of protons

Back 6

Atomic number

Front 7

______ - ________= neutrons

Back 7

atomic mass- protons = neutrons

Front 8

_____ has lost an electron and there fore has a positive charge

Back 8

cation

Front 9

______ has gained an electron and therefore has a negative charge

Back 9

anion

Front 10

Mg (+2) is a ______

Back 10

cation

Front 11

Cl (-1) is a ________

Back 11

anion

Front 12

What is the formula to find the charge of an ion (the little number next to the symbol at the very top right corner)

Back 12

# of protons- # of electrons

Front 13

The +/- charge at the top right of the symbol means whether the atom is a ____ or ____.

Back 13

cation(+) or anion(-)

Front 14

Steps to calculate Atomic mass (3)

Back 14

1. Change the percentage of the atom to a decimal.

2. Multiply the decimal by the atomic mass for each form of the element.

3. Add up all the numbers

Front 15

When calculation atomic mass get the number of significant numbers from the ______ of the atoms

Back 15

masses

Front 16

In ions the __________ change

Back 16

electrons

Front 17

In Isotopes ________ change

Back 17

neutrons (atomic mass)

Front 18

14

C

6

This is _____

Back 18

Nuclear Notation

Front 19

The top number in nuclear notation is the ____

Back 19

atomic mass

Front 20

The bottom number in nuclear notation is the

Back 20

atomic number

Front 21

Carbon-14

or

C-14 is _________

Back 21

Hyphen notation

Front 22

The number next to the name of the element in hyphen notation is the

Back 22

atomic mass

Front 23

210

Pb

82 is an example of what

Back 23

isotope

Front 24

+2

Mg is an example of what

Back 24

ion

Front 25

________ under go radioactive decay

Back 25

isotopes

Front 26

______ decay: isotopes naturally break down into a smaller element and release particles and energy (radiation) in the process. The reason they break down is that their nucleus is unstable, due to an unfavorable neutron: proton ratio. There are 2 types

Back 26

Radioactive

Front 27

What are the 2 types of radioactive decay

Back 27

Alpha decay and Beta Decay

Front 28

Why do isotopes decay

Back 28

to form a new element with a more stable neutron: proton ratio.

Front 29

_____ decay: releases an alpha(a) particle

Back 29

Alpha

Front 30

What type of nucleus does alpha decay release

Back 30

helium

Front 31

4

He = ________________

2

Back 31

alpha particle

Front 32

238 4 234

U ------> He + Th

92 2 90

What is going on here?

Back 32

Alpha decay

Front 33

In alpha decay, beta decay, electron capture, and positron emission the mass # and atomic # are ______ (______)

Back 33

conserved (meaning they get added like the equation)

Front 34

____ decay: a neutron in the original atom decays to form a proton and an electron

Back 34

beta

Front 35

0

e = ________

-1

Back 35

beta particle

Front 36

210 0 210

Pb ----------> e + Bi

82 -1 83

What is going on here?

Back 36

Beta Decay

Front 37

Both types of decay release _________ radiation in the process.

Back 37

Gamma (Y)

Front 38

Gamma radiation is pure energy, not a particle, so it is _________ represented in the equation

Back 38

not

Front 39

What type of radiation is this?

More massive

Cause the most damage over a short range

Least able to penetrate surfaces; stopped by a piece of paper

Back 39

Alpha

Front 40

What type of radiation is this?

less massive

cause less damage over a short range

more able to penetrate surfaces; stopped by a thing sheet of aluminum foil

Back 40

Beta

Front 41

What type of radiation is this?

no mall; all energy

cause the least damage over a short range

Most able to penetrate surfaces; stopped by a thick sheet of lead

Back 41

Gamma

Front 42

_____ _____
1 process that unstable atoms can use to become more stable.

(looks like beta decay but flipped)

Back 42

Electron capture

Front 43

During electron capture, an _______ in an atom's inner shell is drawn into the nucleus whee it combines with a proton, forming a neutron

Back 43

electron

Front 44

40 0 40

K + e ----------> Ar

19 -1 18

What is going on here?

Back 44

Electron Capture

Front 45

___ _____

position; antiparticle for an electron; has the same mass as an electron but carries a positive charge

Back 45

positron emission

Front 46

_________ are found in collisions initiated by cosmic rays

Back 46

positrons

Front 47

0

e = _________

+1

Back 47

Positron

Front 48

41 0 41

Ca ----------> e + K

20 +1 19

What is going on here?

Back 48

Positron Emission

Front 49

division

splitting apart

Back 49

fission

Front 50

2 H coming together 2 produce oxygen

Back 50

Fusion