Gr.10 Unit 1 Chemistry Summative Assignment

Group # 17: Halogens

Fluorine
Chlorine
Bromine
Iodine
Astatine
Ununseptium

Group # 1: Alkali metals

Hydrogen
Lithium
Sodium
Potassium
Rubidium
Cesium
Francium

Group # 18: Noble gasses

Helium
Neon
Argon
Krypton
Xenon
Radon
Ununoctium

Group # 2: Alkaline Earth metals

Beryllium
Magnesium
Calcium
Strontium
Barium
Radium

Protons = p+

The Atomic Number = # of p+

Neutrons = n°

Electrons = e-

# of e- = number of p+
(In atom)

Atomic Mass = # of p+ (+) # of e-

Mass Number = # of e- + # of n°

Mass # (-) # of e- = # of n °

Valence shell
is the outer ring of an atom

8 Electrons fit in the outer shell

Octet Rule:
Elements tend to acquire 8 (e-) in the
outer most shell to become stable

Subtopic

Sour taste
 React with some metals to produce H2
 A good conductor of electricity in solution

 Reacts with base to produce salt and water

 React with pH Indicators & change colour

 Blue litmus paper turns red in an acid

 Red Litmus paper stay red in an acid

 Pink phenolphthlalein turns colourless in an acid

 Neutral (green) bromothymol blue turns yellow in an

acid

 Methyl orange turns red in an acid

Contains Hydrogen and one other element

Naming Binary acids

1. Use Hydro as prefix
2. add the main portion of the second element
3. It will end with "ic"

HCl(aq) -----> Hydrochloric acid

For all acids, the number of
hydrogen atoms is equal to the
valence or charge on the

element or radical it is bonding with

Contains Hydrogen, Oxygen
and one other element

They are formed with
polyatomic ions (radical like sulfate)
which react with hydrogen

Naming oxyacids

The radical ending "ate"
is dropped

The ending "ic acid" is added to the stem

Examples

(SO4)^2-
to H
2(SO4)
Sulfate to sulfuric acid

Bases

Examples of bases

Baking Soda
Detergent
Soap and Bath products

https://examples.yourdictionary.com/20-common-examples-of-bases-in-everyday-life.html

A Base is a Compound that
dissolves in water to produce
hydroxide ions (OH-) in solution

Properties of bases

 Are basic or alkaline
 Bitter taste
 Most are solids

 Slippery and soapy to the touch

 A good conductor of electricity in solution

 React with acid to produce salt and water

 Indicators

 Red litmus turns blue

 Blue Litmus paper stay blue

 Colourless phenolphthlalein turns pink

 Neutral (green) bromthyol blue turns blue

 Methyl orange turns yellowish orange

 Cabbage Juice turns blue-green

Naming bases

The name for bases starts with a metal and ends with Hydroxide (OH^-1)

 We use the cross-over rule for the valences
charges but don’t forget the brackets
around the hydroxide

Examples

For ammonium Hydroxide

From the slides

Ionic Compound

Bonds that are formed by transfer of
electrons from one element to the other

Each element (now an ion) will have a
complete octet after the transfer of electrons.

The electrical force between the ions will be opposite with the metal being positivly charged and the gas being negatively charged

Chemical formula

A representation of the kind
and number of atoms in a substance

Formula unit

A chemical formula that shows the
lowest whole number ratio of the
atoms (ions) in an ionic compound.

Polyatomic ions

Groups of atoms that stay together and
carry and overall ionic charge

Also known as Radicals

Bond with a metal to form
an ionic compound

Example

Table salt

NaCl

Sodium chloride

https://chem.libretexts.org/Bookshelves/General_Chemistry/Map%3A_A_Molecular_Approach_(Tro)/03%3A_Molecules_Compounds_and_Chemical_Equations/3.05%3A_Ionic_Compounds-_Formulas_and_Names

Chemical in toothpaste

NaF

Sodium Fluoride

Baking soda

Na(HCO3)

Sodium bicarbonate

Covalent/Molecular
compound

When two or more non-metal elements are combined together, it is a covalent compound/molecular compound

The atoms are held together by covalent bonds which is when the atoms share their valence electrons

Unlike formula units, covalent compounds can have multiple combinations, and not be a fixed ratio

Some elements may be diatomic
(they exist in nature as double bonded naturally)

H ,O ,N ,Cl ,F, Br

Diatomic elements

Examples

mouth wash

Hydrogen peroxide

https://www.pure-chemical.com/blog/list-of-chemicals-in-daily-life/

Water

Hydrogen dioxide

H2O

oxygen

O2

Carbon dioxide

CO

Synthesis

Synthesis reactions occur when two
substances (generally elements)
combine and form a compound.

(Sometimes these are called combination

or addition reactions.)

Basically: A + B = AB

Decomposition

Decomposition reactions occur when a
compound breaks up into the elements or in
to simpler compounds

AB = A + B

Carbonates and chlorates are special case
decomposition reactions that do not go to
the elements.

Carbonates (CO3
2-) decompose to carbon dioxide
and a metal oxide

Single displacement

Single Displacement Reactions occur when
one element replaces another in a compound.
A metal can replace a metal (+)

Balanced Single displacement reaction

a nonmetal can replace a nonmetal (-)

A + BC  AC + B (if A & B are metal) OR
A + BC  BA + C (if A & C are nonmetal)

Double discplacement

Double Displacement Reactions occur when a
metal replaces a metal in a compound and a
nonmetal replaces a nonmetal in a compound

AB + CD  AD + CB

Combustion

occur when a hydrocarbon
reacts with oxygen gas. (Burning)

In order to burn something
you need the 3 things in
the “fire triangle”:

1) A Fuel (hydrocarbon)

2) Oxygen to burn it with

3) Something to ignite the

reaction (spark)

Chemical equations

Reactants

The atoms/ions that will form the product

Products

The sum of the reactant

H2O2