Nomenclature and Lewis Structures

Nomenclature Information

100

What is the difference between ionic and covalent compounds?

Ionic compounds contain metals, and covalent compounds only contain non-metals.

200

For type II ionic compounds, how do we write the name when we’re given the formula?

You split the metal from the rest of the compound, then use the known charge of the non-metal to find the charge of the metal. This must be written in the name after the metal in parentheses using Roman numerals.

300

What are the numbers relating to the prefixes tetra, hexa, septa, and deca?

4, 6, 7, 10

400

When given a name for an ionic compound, how do you know what the charge of your first element is for each type?

For type I, you simply use the fixed charges from the periodic table.

For type II, the parentheses containing Roman numerals after the metal hold the charge of the metal, so you will use that number.

500

List all ten prefixes in order.

Mono, di, tri, tetra, penta, hexa, septa/hepta, octa, nona, and deca 

Nomenclature Formulas

100

Sodium oxide

Na₂O

200

Titanium (III) nitride

TiN 

300

Silicon pentiodide

SiI₅

400

Tin (VI) Chlorite

Sn(ClO₂)₆

500

Triboron nonanitrate

B₃(NO₃)₉

Nomenclature Names

100

CCl₄

Carbon tetrachloride

200

ZnI₂

Zinc iodide

300

Al(ClO₄)₃

Aluminum perchlorate

400

Se₆Br₈

Hexaselenium octabromide

500

Sr₃P₂

Strontium phosphide

Lewis Structures Information

100

What subatomic particle do we use for Lewis structures? How do we find them easily?

Electrons, specifically valence electrons. You use the A numbers for each group, as those are equivalent to the valence electrons.

200

How many valence electrons does N₂ contain?

10

300

Which element is an exception to our typical rules? What are those exceptions? (Hint: this element does not take a key component of Lewis structures)

Hydrogen. It does not go in the center, and it does not take on any lone pairs.

400

How do we satisfy the octet rule if we run out of electrons?

You may a double bond using an outer electron. You should not make a double bond unless you have no other options left.

500

What breaks symmetry?

Lone pairs on the central atom, or differing elements surrounding the central atom.

Lewis Structures Practice

100

What is the VSEPR formula of NH₃?

4,3,1

200

Draw the correct Lewis structure of beryllium chloride.

(I will do this one up on the board to check your answers)

300

What is the bond angle of water?

<<109.5°

400

Determine the molecular geometry of SH₂.

Bent

500

Find the molecular polarity of SO₂Cl_2, then determine the bond polarity between sulfur and chlorine.

Molecular polarity: polar

Bond polarity S-Cl: polar