Chemical foundations

What was the first rule that Dalton claimed in the small hard balls model

Elements are made of tiny particles called atoms

What was the second rule that Dalton claimed in the small hard balls model

All atoms of the same element are identifical

What was the third rule that Dalton claimed in the small hard balls model

Atoms of different elements have different properties

What was the fourth rule that Dalton claimed in the small hard balls model

atoms of one element will combine with other atoms to form compounds.

What was the 5th rule that Dalton claimed in the small hard balls model

Atoms are rearranged during chemical reactions, they are never created nor are they designed.

What does dalton’s theory of small hard ball model look like?

Different type of circle shapes with different shapes inside of them to represent the various elements.

What did JJ Thompson describe the atom as .

he described it as a plum pudding model.

What did the plum pudding model say about the atom.

This model said that the atom was all positive charge with little negative chargers stuck to it.

What did Rutherford discover

The Nuclear model

What did the nuclear model suggest?

The positively charged area was very small but massive enough to defect the alpha particles, we call this “area” the nucleus with a positive charge.

Do protons have a positive or negative charge

Positive

What other subatomic particles does the proton share the same mass with

Neutron.

What part of the element is the proton the same as

The atomic number

What type of charge does a neutron have

Neutral charge

Is the mass for a neutron the exact same?

No, in fact the neutron tends to be slightly heavier.

What is the purpose of a neutron?

Neutrons act as the glue that holds together the nucleus.

What is a characteristic that the nucleus defines

too many or too few neutrons can result in nuclear instability/radioactive decay.

What type of charge does an electron have

Negative charge in a neutral atom

How is the mass of the electron compared to the proton

The mass of an electron is 2000 times lighter.

What does the electron do In the atom location wise

It is moving around the nucleus at the near speed of light.

Define isotope

A different version of the same chemical element that has the same number of protons but a different number of neutrons.

Whats the result of different neutrons on an atom

Different mass number and potential instability.

What can the atomic mass minus mass number get you

Mass excess, how much actual mass deviates from a whole number due to nuclear binding energy.

What happened when an atom gains or loses an electron

It takes on a charge and becomes an ion

What is the charge of an ion determined by

the number of electrons gained or lost.

Define Alpha decay

A type of radioactive decay where a nucleus emits an alpha particle, an alpha particle is essentially a helium nucleus, so it's a group of two protons and two neutrons.

Define Beta decay

A type of radioactive decay where a nucleus emits a beta particle, if an electron is involved, the number of neutrons decrease by one and the number of protons increase by one.

Define gamma decay

The nucleus changes from a higher-level energy state to a lower level. In the process, electromagnetic radiation is emitted (gamma ray).

what do scientists call the rate of radioactive decay

radionuclides

What is a half life

the amount of time required for the disintegration of the one-half of the radioactive atoms that are present when measurement starts.

Using a graph how do you find how much material will be left after a number of half lives.

(1/2)^n

Nuclear fission

Splitting a heavier nucleus into nuclei with small mass numbers

Nuclear fission

Splitting a heavier nucleus into nuclei with smaller mass numbers

Nuclear fusion

combining two light nuclei to form a heavier more stable nucleus

Define the average atomic mass

The weighted average of the masses of the isotopes of that element

What two things do we use to determine the AMU

Isotope mass and the percent abundance of isotope or decimal fraction of isotope.