Chemistry Unit #03

What happens to Atomic Radius across a period? Why?

It decreases because more protons and the same amount of orbitals means a greater pull.

What happens to Atomic Radius down a group? Why?

It increases because more orbitals means more electrons that are further away from the nucleus.

What happens to Ionization Energy across a period? Why?

It increases because a greater pull from the protons means it is harder to remove electrons.

What happens to Ionization Energy down a group? Why?

It decreases because electrons further from the nucleus are easier to remove.

What happens to Ionic Radius across a period?

It decreases same reason as atomic radius.

What happens to Ionic Radius down a group?

It increases same reason as atomic radius.

What happens to an atom’s size when the atom is negatively charged (Anion)? Why?

The atom becomes larger because there is a larger pushing force from more electrons on a lesser amount of protons.

What happens to an atom’s size when it is positively charged (Cation)? Why?

It gets smaller because there is a greater pull on fewer electrons by more protons.

What happens to Electronegativity moving across a period? Why?

Electronegativity increases moving across a period because electrons are more likely to be attracted to an atom with a smaller atomic radius.

What happens to Electronegativity moving down a group? Why?

Electronegativity decreases because electrons are less likely to be attracted to an atom with a smaller atomic radius.

Name the three states of matter.

Solid, liquid, gas.

What is the name for group 1? How many valence electrons do all atoms in this group have?

Alkali metals. 1 valence electron.

What is the name for group 2? How many valence electrons do all atoms in this group have?

Alkaline earth metals. 2 valence electrons.

What is the name for group 17? How many valence electrons do all atoms in this group have?

Halogens. 7 valence electrons.

What is the name for group 18? How many valence electrons do all atoms in this group have?

Noble gases. 8 valence electrons.

What are the types of elements?

Representative and transition.

What are the classes of elements? What are these types’ characteristics?

Metals, nonmetals, metalloids. Metals are shiny, malleable, good conductors of heat and electricity. Nonmetals are brittle when solid, poor conductors of heat and electricity, low melting and boiling points. Metalloids have characteristics of metals and nonmetals, semiconductors.

What are the properties of Alkali metals?

Highly reactive, soft, low melting points, largest atomic radii.

What are the properties of alkaline earth metals?

Good conductors, highly reactive

Boron group characteristics

3 valence electrons

Transition metals vs. inner transition metals

Transition metals have their valence electron in the outermost d orbital while inner transition metals have their valence electron in the inner f orbital.

Transition metals and inner transition metals are quirky. Why?

Unique electron configs means readily lose electrons.

What is Planck’s constant?

6.626×10^-34

How to calculate frequency given energy?

v=E/h

How to calculate frequency given wavelength?

v=c/λ

How to determine energy given frequency?

E=hv

What do we always do when wavelength is involved?

Convert to meters!!!!