Chemistry: Periodic Table, Elements, and Nuclear Chemistry

What is the number at the top of an element called

Atomic number

What does the atomic number denote

Amount of protons and electrons

What is the letter in the middle of an element

The elemental symbol

What is the number under the elemental symbol

Atomic mass

Name of horizontal rows

Periods

How many periods are there

7

How many families are there

8

Vertical rows on the periodic table

Groups

How many groups are there

18

What do the families tell you about the electrons of elements in them

they tell you how many valence electrons each group has.

Where are metals located on the periodic table

Left side of the staircase

What is the rule for metallic character

As you move further to the left and down their is more metallic character

What are the characteristics of metals

Conductors, Malleable, Ductile, Lustrous

Where are non metals found on the periodic table

On the right side of the staircase

What is the rule for non-metals

as you move to the right and up, there is more non-metallic character

What are the characteristics of non metals

Low boiling points, brittle, dull, good insulators

What are metalloids?

Elements that have properties of metals and non-metals

Where are metalloids found

ALong the staricase

What is an example of a metalloid

Silicon

What is the special name of group 1

Alkali Metals

What is the special name of group 2

Alkaline Earth Metals

What is the special name of group 17/7

Halogens

What is the special name of group 16/6

Chalcogens

What is the special name for group 18/8

Noble gases

A positively charged subatomic particle found in the nucleus of an atom

Proton

A subatomic particle with no charge found in then nucleus of an otma

Neutron

a negatively charged sub-atomic particle

Electron

What is the mass number in isotope notation 

The total number of protons and neutrons

How do you find the amount of neutrons in an atom

Subtract the protons from the mass number

What is an isotope

atoms that have the same number of protons but a different number of neutrons 

A weighted average of the masses of an element’s isotope

Average Atomic Mass

The percent of an element in nature that is that isotope

Percent abundance

One half the distance between the nuclei of two atoms of the same element when the atoms are joined. 

Atomic radius

What effects the atomic radius

Size of an atom

Ionization energy

The energy required to remove an electron from an atom

Electron Affinity

How much an atom wants an electron

Electronegativity

the ability of an atom of an element to attract electrons when the atoms is in a compound.

What do most periodic property trends result from

The Shielding Effect

How does the shielding effect work

Electrons are attracted to nucleus by electric charge. Electrons on the inner levels shield the outer electrons from

the nucleus’s gravity.

Any atom or group with a positive charge

cations

Any atom or group with a negative charge

anions

Why is atomic radius larger going down.

Higher energy levels have larger orbits + shielding

Why is the atomic radius smaller to the right.

Increased nuclear charge without additional shielding.

Why does ionization eneryg decrease going down.

Shielding effect causes electrons that are further to be less attracted and easier to remove. 

Why does the ionization energy increase going to the right

Stable electron configurations don’t want to lose electrons.

Why does electron affinity decrease going down

More total electrons will repel each other + shielding.

WHy does electron affinity increase to the right

The closer to a full outer level, the more an atoms attracts electrons.

Which is the most electronegative

fluorine

Why do you use electronegetive trends not for noble bonds

because noble gases don’t make bonds

Why does electronegativity decrease going down

Shielding

The process by which nuclei emit particles and rays

Radioactivity

The energy rays and particles given off by a radioactive source

Radiation

An isotope that has an unstable nucleus undergoes radioactive decay

Radioisotopes

Stability of an isotope depends on what

p to