Chapter 4 Flashcards
Identify the characteristics of the alkali metals.
aka group 1
- low ionization energy
- very reactive with water
- readily forms ionic compounds
Identify the characteristics of the alkaline earth metals.
similar to group 1, except they don’t have as low of an ionization energy and they are not as reactive with water however - they become more reactive the further down the column
Identify the characteristics of the halogens.
- highly reactive with metals
- very electronegative
- good oxidizing agents
Describe the periodic trend for atomic size.
Right to left and DOWN the periodic table = bigger size
Describe why size decreases when an atom has more protons.
Effective nuclear charge - the protons will “suck” the surrounding electrons
Effective nuclear charge ______ when size ______
increases, decreases - or vice versa; inverse relationship
Isoelectronic Series
a group of ions or atoms that are from different elements, but have the same total number of electrons as each other
Ionization Energy
The amount of energy needed to strip 1 electron from an atom
Describe the periodic table trend for ionization energy
Increases as you go from left to right and UP the periodic table; includes noble gases
What are the exceptions for the ionization energy trend on the periodic table?
Nitrogen has a larger ionization energy than oxygen
Be has a larger ionization energy than boron
T/F? It is more favorable to have a full filled 2s orbital than a half filled.
TRUE
Which has a larger atomic radius? O2- or O2? Explain why.
O2 is larger
Atoms become smaller when they become ions; lose electrons = smaller, gain electrons = bigger
Which atom has the highest electron affinity?
a) Fluorine
b) Chloride
c) Helium
d) Francium
B
recall that electron affinity follows the same exact trend as electronegativity (with F being the most electronegative) - except with the trend of electron affinity - Cl has the most affinity for electrons!
