Test 1 Flashcards
Electron Affinity
Closest to Fluorine, increases from left to right and bottom to top. (Atom that wants an electron the most, (Halogens)).
Ionization Energy
First Column has lowest ionization energy. Cs has lower energy than Li. The amount of energy to remove one electron from an atom. Opposite of electronegativity. Atoms with low IE are happy to give up electrons.
Periods
Horizontal Rows
Groups
Vertical Columns
Cations
Smaller than their neutral counterparts. The positive charged nucleus pulls electrons in. Li> Li+
Anions
Greater in radius than their neutral counterparts. Not enough protons to pull down on the electrons.
Isoelectronic Ions
All have same number of electrons. Smallest in radius have most positive charge because protons pull down the electrons. Ca2+, Ar, S2-
Z effective
The effective nuclear charge that an electron feels when shielded by other electrons. Increasing atomic number means increasing Zeff
As you move right across the P Table what happens
- Increasing atomic number
- Increasing Z eff
- Decreasing Radius
- Increasing eN
- Increasing electron affinity
- Increasing ionization energy
Atomic Radius
As Zeff increases atomic radius decreases. Atomic radius decreases as you move right and increases as you move down.
Electronegativity
Propensity of an atom to attract electrons. Fluorine is most eN. Halogens and anything close to fluorine are highly eN
As you move from top to bottom of the P table
1.Increasing principle quantum number (n)
2. No zeff trend
3. Increasing radius
4. Decreasing eN
5. Decreasing electron affinity
Decreasing ionization energy
Paramagnetic
Has at least one unpaired electron, and is magnetic
Diamagnetic
Every electron is paired up and is not magnetic.
Mg electron configuration
Mg: [Ne] 3s^2
Mg^+:[Ne]3s^1
Mg^2+:[Ar]
