Metals and Metal Compounds Unit E

Do Now: What characteristics does a metal have? What is an example of a metal?

Metals Periodic Table – contains all elements Elements – a substance made of 1 type of atom Metal – an element that is usually a good conductor – Contains physical and chemical properties

How do you tell if it is a metal? Physical Properties – Malleability, conductive, colour, sonorous, melting point, boiling point Chemical Properties – A reaction with another substance, ex. Iron rusting

The Periodic Table

Types of Metals – Group 1 Alkali Metals – very reactive, usually found combined with another substance

Group 2 Alkaline Earth Metals – Reactive, harder than alkali metals, usually combined with other elements

Groups 3-12 Transition Metals – most common metals, good conductors of electricity. Hard and shiny

Other metal groups: Metalloids Lanthanides Actinides Post – Transition Metals

Do Now: Name each of the following and classify what type of metal it is: – Mg – Al – Cs – Fe – Sn – Ge

Making Salts Salt – A substance produced when an acid reacts with a base – Sulphates – Chlorides – Nitrates

What is an ACID? pH less than 7 Neutralizes bases Forms H + ions in solution Corrosive-reacts with most metals to form hydrogen gas Good conductors of electricity

Common Acids HCl- hydrochloric- stomach acid H 2 SO 4 - sulfuric acid - car batteries HNO 3 – nitric acid - explosives HC 2 H 3 O 2 - acetic acid - vinegar H 2 CO 3 -carbonic acid – sodas H 3 PO 4 - phosphoric acid -flavorings

What is a BASE? pH greater than 7 Feels slippery Dissolves fats and oils Usually forms OH- ions in solution Neutralizes acids

Weak vs. Strong Bases Weak Bases: ammonia; potassium carbonate, sodium carbonate Strong Bases: sodium hydroxide; sodium phosphate; barium hydroxide; calcium hydroxide

Common Bases NaOH- sodium hydroxide (LYE) soaps, drain cleaner Mg (OH) 2 - magnesium hydroxide-antacids Al(OH) 3 -aluminum hydroxide-antacids, deodorants NH 4 OH-ammonium hydroxide- “ammonia”

What is a SALT? A salt is a neutral substance produced from the reaction of an acid and a base. Composed of the negative ion of an acid and the positive ion of a base. One of the products of a Neutralization Reaction Examples: KCl, MgSO 4, NaNO 2

Metal + Acid = A Salt Mg + HCl → Zn + HCl → Fe + HCl → Sn + HCl → Cu + HCl →

Write out the equations

Do Now: Answer questions a-d on page 64

Acids and Bases Pure metal + acid = salt + hydrogen gas Base + Acid = salt + water – Bases are a metal with: Oxides Hydroxides Carbonates

Identify the following: MgO HNO 3 KOH Ca(OH) 2 HCl NaOH CaCO 3

Name the following: HNO 3 KOH Ca(OH) 2 HCl NaOH MgO CaCO 3

Neutralization Neutralization – Reaction between an acid and a base. What is the pH of a base? What is the pH of an acid? What is the pH after neutralization?

Reactions Acid + metal oxide → a salt + water Acid + metal hydroxide → a salt + water Acid + metal carbonate → a salt + water + carbon dioxide

entration entration

Properties of Acids: they taste sour turn litmus paper red react with certain metals to yield hydrogen gas.

Properties of Bases: they taste bitter turn litmus paper blue feel slippery

Common Acids and Bases at Home: Vinegar Baking soda Soap Ammonia Soda bases-found-homes.html bases-found-homes.html

Do Now: Look at your results from yesterdays titration lab. Compare your acid and base. Which is stronger or are they similar? Why?

Need to Know Chemical Formulas: Products: – Water H 2 O – Hydrogen Gas H 2 – Carbon Dioxide CO 2 Acids: – Hydrochloric Acid HCl – Sulphuric Acid H 2 SO 4 – Nitric Acid HNO 3

Reactions with a Metal: Hydrochloric Acid + Metal → Metal chloride + hydrogen gas Sulphuric Acid + Metal → Metal sulphate + hydrogen gas Nitric Acid + Metal → Metal Nitrate + hydrogen gas

Reactions with Metal Oxides: Hydrochloric Acid +Metal Oxide → Metal Chloride + Water Sulphuric Acid + Metal Oxide → Metal Sulphate + Water Nitric Acid + Metal Oxide → Metal Nitrate + Water Oxide = Metal and only oxygen – MgO – Na 2 O – Al 2 O 3

Reactions with Metal Hydroxides: Hydrochloric Acid + Metal Hydroxide → Metal Chloride + Water Sulphuric Acid + Metal Hydroxide → Metal Sulphate + Water Nitric Acid + Metal Hydroxide → Metal Nitrate + Water The biggest change with a hydroxide from an oxide, the final equation WILL need to balanced! Metal Hydroxide = Metal with an oxygen and hydrogen (OH) – NaOH – Al(OH) 3 – Ba(OH) 2

Reactions with Metal Carbonates: Hydrochloric Acid + Metal Carbonate → Metal Chloride + Water + Carbon Dioxide Sulphuric Acid + Metal Carbonate → Metal Sulphate + Water + Carbon Dioxide Nitric Acid + Metal Carbonate → Metal Nitrate + Water + Carbon Dioxide Carbonates will ALWAYS produce carbon dioxide! These reactions will usually need to be balanced! Metal Carbonate = Metal with carbon and oxygen (CO 3 ) – CaCO 3 – MgCO 3 – Na 2 CO 3

Activity: Complete the worksheet for practice

Do Now: Complete and balance the following reactions: 1._____ + NaOH → NaCl + ________ 2.H 2 SO 4 + Al 2 (CO 3 ) 3 → Al 2 (SO 4 ) 3 + ___________ 3._______ + Zn → Z n (NO 3 ) 2 + ____________ 4.HCl + _________ → KCl + H 2 5.______ + Ba(OH) 2 → Ba(NO 3 ) 2 + __________

Use of Salts Sodium Chloride – table salt

Fertilizers Fertilizer – Nutrients that can be added to a soil if needed – Many are made up of : Nitrogen (N) Phosphorus (P) Potassium (K)

NPK Fertilizers often have 3 numbers, representing the percentage of each element inside

NPK Nitrogen provides plants with the ability to produce more chlorophyll, which in turn allows plants to grow quickly Phosphorous aids in root development and increases flowering ability and bloom size Potassium has many functions: – It guards the plant against diseases – Aids in drought protection and cold tolerance. – Serves a role in improving root development – helps in the process of photosynthesis

How much of each? Why is the total percent not 100?

Activity: Open your books to page 67: Answer questions 1 and 2 Besides, fertilizers and table salt, what other places do you see salts being used?