Studied by 7 people
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?
Note
Flashcard