TSNF Unit 1 AP Chemistry

Protons are equal to an atom's

atomic number

Electrons are equal to:

the protons in a neutral atom

What comes after 6s?

4f

% composition by mass for a pure compound _____________

does not change

What is the electron configuration order?

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6

anions are:

negative, and gained electrons

The molecular formula for a compound is

a whole # multiple of the empirical formula ratio

Elements in the same ____________ have similar chemical and physical properties.

Group/family (column)

What type of elements are on the left side of the zig-zag line?

Metals

What type of elements are on the right side of the zig-zag line?

Non-Metals

What type of elements are in group one of the periodic table?

Alkali Metals

What type of elements are in group two of the periodic table?

Alkaline Earth Metals

What type of elements are in group seventeen of the periodic table?

Halogens

What type of elements are in group eighteen of the periodic table?

Noble Gases

charge by column:

+1, +2, +3, skip, -3, -2, -1, 0

What does a larger binding energy mean?

stronger coulombic attraction

Binding energy increases as number of ______________ increases

protons

Binding energy is greatest for electrons that are ____________________ to the nucleus

closest

In a PES graph, what does a higher peak represent ?

more electrons in that sublevel

you can determine the valence electrons by:

column in the periodic table

anions (−) are _______________ than their atoms

larger

WHY are anions larger than their atoms?

adding extra electrons increases electron-electron repulsions.

you can determine the charge by:

column in the periodic table

valence electrons by column:

"1, 2, skip a few, 3, 4, 5, 6, 7, 8"

mass spectroscopy graphs measure:

atomic masses of isotopes

Cations (+) are _______________ than their atoms

smaller

Why are cations (+) smaller

since you are removing valence electrons that are farther from the nucleus

When an electron is in a higher the energy level it's ________

farther away from the nucleus and therefore has less Coulombic attraction to the nucleus and is therefore easier to remove (...it has a lower 1st ionization energy.)

Moving across a row on the periodic table ________________________

the protons and Zeff (effective nuclear charge) increases, therefore the valence electrons are more attracted to the nucleus, therefore the atomic radius decreases and the ionization energy and electronegativity increases

electronegativity increases...

up and to the right

ionization energy increases

up and to the right

atomic size increases

down and to the left

In what order should the valence electrons be removed?

HIGHEST NUMBERED FIRST! The p-orbital first and the s-orbital second. The d-orbital third if necessary.

isotopes of an element have the same number of _______, but different numbers of ________.

protons, neutrons

Empirical formula rhyme

→ % to mass, mass to mole, divide by small, multiply until whole...Get the simplest whole # ratio of the moles (or atoms) in the compound

When writing the electron configuration for a cation, what should be done first?

Remove the valence electrons

What does 5f come after?

7s

cations are:

positive, and lost electrons

mass number - _____________ = neutrons

protons