Atoms and Nuclear Chemistry

The smallest part to which an element can be divided yet still be that element, building blocks of all matter

Makeup the nucleus, has a positive charge; 1 amu

Part of the atom with no charge; makes up the nucleus; 1 amu

Negatively charged part of the atom; in the electron cloud outside the nucleus

Centre of the atom; small and dense; contains protons and neutrons

Atoms with the same number of protons but a different amount of neutrons

Atomic #- 17
Mass #- 37
# of protons- 17
# of electrons- 17
#of neutrons- 20

Weighted average of all of an atoms isotopes

(Mass)(%)/100 or (mass)(decimal)

Electrons, rearrange themselves to form a compound

Changes the atom’s nucleus and you get a different element

The nucleus of an atom is unstable because of the proton to neutron ratio

83

Spontaneous process that occurs when an unstable nucleus gives off energy to become stable

Energy given off, waves and particles capable of traveling the speed of light

X-rays, UV rays, microwaves, radio waves

Large and slower moving particles, damaging if digested, can’t penetrate far

Paper or skin

2 protons and 2 neutrons which is a helium nucleus

Fast moving electrons with a small mass and farther penetration than alpha

Thin metals and protective clothing

Neutron is converted to a proton and the negative becomes a beta particle and adds positive to atomic number

Neutral; penetrate far and travel at the speed of light

Thick lead or concrete

Particle with the same mass as an electron but with a positive charge;

Changes a proton to a neutron

Emits a bundle of energy

Used to detect radiation and tells you how much radiation you are absorbing

The splitting of a nucleus into smaller fragments

Heavier atoms go through this for stability

Large amounts

In nuclear power plants and atomic bombs

Combining atoms to make a larger atom

Every element greater than helium

Greek chemist, Believed in atoms and matter

In atoms and that they were the smallest particles, compounds, and he gave the modern atomic model

The electron and the plum pudding model

The nucleus and protons(later) did gold foil experiment

The neutron

Ernst Rutherford

Number of protons and electrons

Total number of protons and neutrons

Atomic number

AR=IA(1/2)^h

Time required for half of a radioactive isotope nuclei to decay into its products

The smallest part to which an element can be divided yet still be that element, building blocks of all matter

Makeup the nucleus, has a positive charge; 1 amu

Part of the atom with no charge; makes up the nucleus; 1 amu

Negatively charged part of the atom; in the electron cloud outside the nucleus

Centre of the atom; small and dense; contains protons and neutrons

Atoms with the same number of protons but a different amount of neutrons

Atomic #- 17
Mass #- 37
# of protons- 17
# of electrons- 17
#of neutrons- 20

Weighted average of all of an atoms isotopes

(Mass)(%)/100 or (mass)(decimal)

Electrons, rearrange themselves to form a compound

Changes the atom’s nucleus and you get a different element

The nucleus of an atom is unstable because of the proton to neutron ratio

83

Spontaneous process that occurs when an unstable nucleus gives off energy to become stable

Energy given off, waves and particles capable of traveling the speed of light

X-rays, UV rays, microwaves, radio waves

Large and slower moving particles, damaging if digested, can’t penetrate far

Paper or skin

2 protons and 2 neutrons which is a helium nucleus

Fast moving electrons with a small mass and farther penetration than alpha

Thin metals and protective clothing

Neutron is converted to a proton and the negative becomes a beta particle and adds positive to atomic number

Neutral; penetrate far and travel at the speed of light

Thick lead or concrete

Particle with the same mass as an electron but with a positive charge;

Changes a proton to a neutron

Emits a bundle of energy

Used to detect radiation and tells you how much radiation you are absorbing

The splitting of a nucleus into smaller fragments

Heavier atoms go through this for stability

Large amounts

In nuclear power plants and atomic bombs

Combining atoms to make a larger atom

Every element greater than helium

Greek chemist, Believed in atoms and matter

In atoms and that they were the smallest particles, compounds, and he gave the modern atomic model

The electron and the plum pudding model

The nucleus and protons(later) did gold foil experiment

The neutron

Ernst Rutherford

Number of protons and electrons

Total number of protons and neutrons

Atomic number

AR=IA(1/2)^h

Time required for half of a radioactive isotope nuclei to decay into its products