periodic table stuff

group/family

a section down the periodic table

period

a section across the periodic table

Atomic radius increases...

as you go down a family because because you add another energy level

Atomic radius decreases...

as you go across a period because there's more attraction between protons/electrons.

1st ionization energy decreases...

as you go down a family because there is a larger atomic radius, meaning there is less attraction on the outer ring

1st ionization energy increases...

as you go across a period because there is more attraction so it's harder to rip an electron away

Ionic radius increases...

in atoms that gain an electron. The more electrons, the larger the radius. The size goes up because electrons repel each other more

Ionic radius decreases...

in atoms that lose an electron. The more lost means the smaller the ionic radius. Electrons are attracted to the nucleus because of positive charge, making the radius smaller

electronegativity increases...

as you move across a period because the number of charges on the nucleus increases. That attracts the bonding pair of electrons more strongly.

electronegativity decreases...

as you move down a family because atomic number increases down a group, and thus there is an increased distance between the valence electrons and nucleus, or a greater atomic radius

Aufbau Principle...

states that in the ground state of an atom or ion, electrons fill subshells of the lowest available energy, then they fill subshells of higher energy. For example, the 1s subshell is filled before the 2s subshell is occupied.

Hunds Rule

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin

pauli exclusion principle

no two electrons in the same atom can have identical values for all four of their quantum numbers. No more than two electrons can occupy the same orbital and two electrons in the same orbital must have opposite spins

planck's constant

6.63 * 10 ^-34 J*s

ion

an atom or group of atoms in which the number of electron s is different from the number of proton s. If the number of electrons is less than the number of protons, the particle is a positive ion, also called a cation.

atom

any particle of matter at its most basic level which contains at least one proton

element

a fundamental item that can't be easily broken into smaller pieces

the radius gets larger

as you move down a group

the larger the radius

the more energy levels you have

the radius gets smaller

as you move across a period

the more they're pulled toward the nucleus

the more valance electrons

no new energy levels are added

as you move across a period

protons increase

as you move from one element to the next across a period

with more rings, there is less of a pull

Why do you think an increase in atomic radius would result in a lower ionization energy?

with less rings, there is more of a pull

Why do you think a decrease in atomic radius would result in a greater ionization energy?

If it's smaller it’ll attract more electrons

How do you think the size of an atom will affect its ability to attract additional electrons?

Upper left region

highest electron affinity

Far left column

largest atoms

Lower left region

highest ionization energy

Upper right region

smallest atoms

Far right column

highest ionization energy

Lower right region

lowest electron affinity

because it's being pulled into the nucleus

Why does the atomic radius decrease as electrons are added to a shell?

because you’re adding another energy level

Why does the atomic radius increase as you go from the top to the bottom of a chemical family?