Chapter 9 Note guide to go with Powerpoint

1. Chapter 9 Note-taking Guide
Name________________________________________________
Monoatomic Ions

Mono means ________________.

When the metals in groups 1A, 2A and 3A lose electrons, they form
_________________ with positive charges _________________ to their
_________________________.

They keep their names and just put the word _____________________ after it.

____________________ tend to gain electrons to form
_____________________.

The charge of any anion is determined by _____________________ 8 from their
group number.

Elements in group _____________ have a -1 charge and so on.

Their names will have the ending ___________________

For example, oxide, nitride, phosphide….etc
Ions of Transition Metals

The metals of groups 1B-8B form more than one _________________ with
different charges.

The charges of the cations of many ________________________ metal ions must
be determined from the number of electrons lost.

To name these ions, a ____________________________ is used in parentheses
after the name of the element.

For example, Fe+3 would be called iron(III).

2. Polyatomic Ions

Some ions, called ________________________________, are composed of more
than one atom.

The names of polyatomic ions end in _________________ or
_________________.

There are three other ions that have different endings ___________________,
_________________________ and _________________________.

All ions with ______________________ in them end with an –ite or an –ate.

Refer to your polyatomic table for the names and charges.
Let’s Practice!

Write the name for the following:

Ca+2

Fe+2

Cu+1

Li2CO3

NH4+

3. 
NO3-

Br-

NH4NO3
Writing Formulas for Ionic Compounds

A __________________________________ is composed of
_____________________ elements and can be either ionic or molecular.

To name any binary ionic compound, place the __________________ first and
then the ____________________ name.

To write a formula for a binary compound, write the symbol of the cation and
then the anion.

Add whatever ___________________ are needed to
________________________ the charges.

BALANCING THE CHARGES IS IMPORTANT!!!!
Balancing Charges Using the Crossdown Method

Write the ________________ first with its ________________.

Then write the _________________ with its ________________.

4. 
The ________________ of one ion becomes the __________________ for the
other ion.

You __________________ them down.

If the charges _____________________, then no numbers are needed.

Remember, each compound wants to have a ________________ charge of
_______________.
Let’s Practice!

Write the formulas for the following binary compounds.

Barium sulfide

Calcium nitride

Lithium oxide

Copper(II) iodide

Iron(III) oxide
Compounds with Polyatomic Ions

Write the ________________ and charge for the cation.

5. 
Write the _____________________________ and the charge.

_____________________ the charges.

Remember, they must balance to _______________.

Pretend the polyatomic ion is ________________ atom.

If more than one polyatomic ion is needed, put _____________________ around
the polyatomic formula.

REMEMBER TO REDUCE ALL FORMULAS IF THEY CAN BE REDUCED!
Let’s Practice!

Write the formulas for the following:

Calcium nitrate

Sodium carbonate

Calcium phosphate
Naming and Writing Formulas for Covalent (Molecular) Compounds

The ____________________ in the name of the binary compound tells how many
atoms of each element are present in the molecule. (see table 9.4)

The _____________________ for all the compounds is _________________.

6. 
Use the ______________________ in the name to tell you the
___________________ of each element in the formula.

Write the correct symbols and the appropriate _____________________.

7. LET’S PRACTICE!

Write the names/formulas of the following compounds.

CS2

Cl2O7

NI3

Carbon tetrabromide

Diphosphorus trioxide
Naming and Writing Formulas for Acids

An ___________________ is a compound that contains one or more
_____________________ atoms and produces hydrogen ______________ when
dissolved in water.

When the name of the anion ends in ____________________, the acid name
begins with the prefix _____________________ and has the suffix
___________________ and ends in acid.

8. 
When the anion name ends in ___________________ the acid name ends in
___________________ followed by acid.

When the anion name ends in ___________________, the acid name ends in
__________________ followed by acid.
LET’S PRACTICE!

Write the name/formula for the following acids:

HBr

H2SO4

Hydrochloric acid

Carbonic acid

HNO2
The Laws of Definite and Multiple Proportions

The _________________________________________________________ states
that in any sample of a chemical compound, the _______________________ of the
elements are always in the same __________________________.

9. 
They will always _______________________ in simple
__________________________ ratios.

The _________________________________ states that whenever two elements
form more than one compound, they will be in simple
________________________________ ratios.
Word Equations

Symbols to remember:

_____________________ means yield or produces or makes, it’s like an =sign
in math

_____________________ means add the compounds together

A ______________________ above the arrow, means ____________________ is
added.

___________ means solid or precipitate, _______________ means aqueous or
dissolved in water, ________________ means gas, ______________________ means
liquid.

Reactants must __________________ the products. No random compounds!!
LET’S PRACTICE!

1. Hydrogen gas and oxygen gas combine to form liquid water.

2. Methane gas (CH4) and oxygen gas combine to form carbon dioxide gas and
liquid water.

10. 
3. Solid Ammonium carbonate and dissolved calcium nitrate are mixed together.
Dissolved Ammonium nitrate and solid calcium carbonate are made.