Chemistry Exam

b) PBSO₄

B) water and oxygen

D) all of the above

B) -ate

True

False

False

False

False

Th nucleus contains protons and neutrons in a heavy, dense positive core that contains the mass of the atom. Outside the nucleus, atoms orbit in defined orbits in the electron shells.

Bohr-Rutherford diagrams visually show the make-up of the nucleus, and every electron orbit outside. A Lewis Dot diagram uses the symbol for the element, surronding by the valence shell only.

• Metals are solid, non-metals are solid/liquid/gas
• Metals are conductors, non-metals are insulators
• Metals are shiny, non-metals are dull
• Metals have extra valence electrons, non-metals don't have enough

Physical and chemical properties are directly related to the number of valence electrons. Elements with the same number of valence electrons will react basically the same. Depending on how far the valence electron is from the nucleus (what electron shell), it becomes more and more reactive. The less electrons an element needs to lose/gain makes it more reactive.

An atom that has gained or lost electrons.

An atom that once had 1-3 electrons, but lost them to form a positive ion.

An atom that once had 5-7 valence electrons, but gained more to form a negative ion.

• Positive Ion - cation
• Negative Ion - anion

• Metals commonly lose electrons to become cations. Non-metals commonly gain electrons to become anion.
• These two opposites attract, and electrons are transferred between the two. A compound is formed.

It will dissociate into its ions, and be able to conduct electricity.

The name of the metal element is written first, unchanged. The name of the non-metal element is written second with the ending changed to "ide". eg. Lithium oxide

The name of the metal is written first with a roman numeral in brackets afterward, indicating the positive charge of the metal. The non-metal ending is "ide".

Workplace Hazardous Materials Information System

Material Safety Data Sheet

• Nitrate ion NO₃^-
• Nitrite ion NO₂^-
• Hydroxide OH^-
• Hydrogen carbonate (bicarbonate) HCO₃^-
• Chlorate ion ClO₃^-
• Carbonate ion CO₃^2-
• Sulfate ion SO₄^2-
• Phosphate ion PO₄^3-
• Ammonium ion NH₄⁺

• Nitrate ion
• Nitrite ion
• Hydroxide
• Hydrogen carbonate (bicarbonate)
• Chlorate ion
• Carbonate ion
• Sulfate ion
• Phosphate ion
• Ammonium ion

Name the metal first, unchanged. Name the polyatomic ion second, unchanged. (If it is ammonium, ammonium comes first, then the metal changes to an ending of "ide")

A neutral group of atoms, called molecules, are formed when non-metal elements chemically join together.

• Ionic compounds dissociate when dissolved, moleculars do not
• Ion compounds conduct electricity, moleculars do not
• Molecular - non-metals, Ionic - metal & non-metal
• Ionic and molecular compounds are neutral

They are formed through the sharing of electrons in the valence shell.

Through the 'combining capacity'. This is also how many electrons an atom needs to gian to complete its valence shell.

Mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca

The element farthest to the left side of the periodic table is written first, unchanged. The second element is changed to "ide". Prefixes are used on both to allude to the number of atoms in the compound (mono is only used on the second element!).

A molecular compound containing two elements, one of which is always hydrogen. Ions are produced when the acid is dissolved in water. Hydrogen is the positive ion, and therefore always written first in the equation.

Normally if it is a gaseous binary compound. If it is in its aqueos acid name, the prefix "hydro" is used, with the ending changed from "ide" to "ic". eg. hydrogen fluoride -> hydrofluoric

An acid containing more than two elements, one of which is hydrogen, the other oxygen. The other element must be a non-metal. They are related to the polyatomic ions.

There is no prefix, the non-metal element is changed to an "ic" ending. eg. H₃PO₄ -> phosphoric acid

• HNO₃ (aq) -> nitric acid
• HNO₂ (aq) -> nitrous acid

An ionic compound containing 3 elements, two of which are hydrogen and oxygen in the form of hydroxide (OH^-).

The metal name is first, unchanged. The second part is hydroxide. eg. LiOH -> lithium hydroxide

N₂O₄

Using either a word equation (reactant and product names) or a chemical equation (balanced reactant and product formulas).

• a) (s)
• b) (g)
• c) (l)
• d) (aq)

4FeS₂ + 11O₂ -> 2Fe₂O₃ + 8SO₂

total mass of reactants = total mass of products

2C₂H₂ + 5O₂ -> 4CO₂ + 2H₂O

The formation of one product from two or more reactants (which can be elements or compounds). eg. A + B -> AB

The splitting of one reactant molecule into two or more products. eg. AB -> A + B

A reaction between a single element and a single compound, where the single element repalces another element in the compound. eg. A + BC -> AC + B

Involves two compounds in which the metals switch places. eg. AB + CD -> AD + CB

This is a special type of double displacement involving an acid and a base, where the products are always a salt and water. eg. HCl + NaOH -> NaCl + H₂O

A synthesis reaction that involves burning a carbon-based fuel (ex. hydrocarbons) with oxygen. Combustion is either complete or incomplete.

A reaction where there is excess oxygen, therefore all the fuel is used. The only products are carbon dioxide and water. eg. C₃H₈ + 5O₂ -> 3CO₂ + 4H₂O

A reaction where there is limited oxygen, therefore there is not enough to completely burn the fuel. The products are water, carbon dioxide, carbon monoxide and solid carbon particles (soot). eg. 2C₃H₈ + 7O₂ -> 2CO₂ + 8H₂O + 2CO + 2C

A scale that measures how acidic or basic a solution is, ranging from 0 - 14. This scale is logarithmic, meaning that a difference of 1 pH is a 10-fold difference in acid concentration.

The concentration of H⁺ or OH^- ions. A strong acid will have a high concentration of hydrogen ions, and a low pH level. Bases are the opposite. A solution with a pH of 7 is neutral because the ion concentrations are equal and balance each other out.

H₂SO₄ + 2NaOH -> Na₂SO₄ + 2H₂O

Industrial plants, coal fire plants, smelting operations, smokestacks emitting sulphur dioxide, cars

• a) gives off protons, low pH level
• b) accepts protons, high pH level

In 1977, acid was slowly added to a lake to explore the effects of acid rain on water ecosystems. In the seven years it ran, the pH level dropped from 6.1 to 5, with organisms slowly dying out. In the end, there were no organisms left and the lake was crystal clear.

B) Cu₃PO₄ - copper (I) phosphate

C) Al(OH)₃

Alkaline Earth Metals

These are compounds made up of two identical atoms. eg. F₂, O₂ etc.