Gr.10 Unit 1 Chemistry Summative Assignment

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Foundation Chemistry UNIT 1

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H2O2

Acid is a coumpound that dissolves in water to produce hydrogen ions (H+) in solutions

Note: aq stands for aqueous or dissolved in water

Lewis dot diagram of Sodium and Chlorine Ions (Full valence orbits)

Sodium Ionically bonding with Chlorine (Electrons moving from sodium to Chlorine)

Lewis dot diagram of a chlorine atom

Gr.10 Unit 1 Chemistry Summative Assignment

Chemical reactions

Chemical equations

Products

The sum of the reactant

Reactants

The atoms/ions that will form the product

Combustion

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)

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

Double discplacement

AB + CD  AD + CB

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

Balanced double displacement equation (without symbols clarifying solid, liquid, gas, aqueous)

Single displacement

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

a nonmetal can replace a nonmetal (-)

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

Balanced Single displacement reaction

Decomposition

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

AB = A + B

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

Synthesis

Basically: A + B = AB

Synthesis reactions occur when two substances (generally elements) combine and form a compound. (Sometimes these are called combination or addition reactions.)

Balanced synthesis reaction

Bonding

Covalent/Molecular compound

Carbon dioxide

CO

oxygen

O2

Water

H2O

Hydrogen dioxide

mouth wash

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

Hydrogen peroxide

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

H ,O ,N ,Cl ,F, Br Diatomic elements

Diagram

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

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

Ionic Compound

Example

Baking soda

Na(HCO3)

Sodium bicarbonate

Chemical in toothpaste

Sodium Fluoride

NaF

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

Table salt

Sodium chloride

NaCl

Polyatomic ions

Bond with a metal to form an ionic compound

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

Also known as Radicals

Formula unit

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

Chemical formula

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

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

Acids and bases

Bases

Naming bases

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

For ammonium Hydroxide

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

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

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

Examples of bases

Baking Soda Detergent Soap and Bath products

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

Acids

Oxyacids

Naming oxyacids

The radical ending "ate" is dropped

The ending "ic acid" is added to the stem

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

Contains Hydrogen, Oxygen and one other element

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

Binary Acids

For all acids, the number of hydrogen atoms is equal to the valence or charge on the element or radical it is bonding with

Naming Binary acids

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

Examples

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

Contains Hydrogen and one other element

Examples of acids

Citrus fruits Aspirin Stomach Acid Vinegar

Properties of Acids

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

Ions

Ions: Atoms with a charge

Polyatomic Ions

Ions that form with two or more atoms

Anions: Atoms with a negative charge

Cations: atoms with a positive charge

Diagrams

Lewis dot diagram

Bohr-Rutherford Diagram

Bohr-Rutherford diagram of a oxygen atom

Perodic table

Subtopic

Atoms

Electrons = e-

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

The noble gasses will always have a filled outer ring

Mass Number = # of e- + # of n°

Mass # (-) # of e- = # of n °

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

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

Neutrons = n°

Protons = p+

The Atomic Number = # of p+

Elements

Common Multivalent Elements

7 Periods and 18 Groups

Group # 2: Alkaline Earth metals

Beryllium Magnesium Calcium Strontium Barium Radium

Group # 18: Noble gasses

Helium Neon Argon Krypton Xenon Radon Ununoctium

Group # 1: Alkali metals

Hydrogen Lithium Sodium Potassium Rubidium Cesium Francium

Group # 17: Halogens

Fluorine Chlorine Bromine Iodine Astatine Ununseptium