Chemistry Unit Review Game

Chapter 1 Anything that has mass and volume is considered to be??? A – Matter An example of this type of change is a change of state. A – Physical change What physical property can be measured numerically? A – Quantitative properites

Qualitative and Quantitative Properties Which of these properties is not a qualitative property: ductility, malleability, magnetism, conductivity, colour? A – Conductivity What quantitative property is the ability to dissolve in water? A – Solubility What qualitative property is the ability to be beaten into sheets? A - Malleability

Dalton’s Atomic Theory – Main Points All matter is made of small particles called atoms. Atoms cannot be created, destroyed, or divided into smaller particles. All atoms of the same element are identical in mass and size, but are different in mass or size from the other elements. Compounds are created when atoms of different elements link together in definite proportions.

Who proposed the “raisin bun” model of the atom? A – J.J. Thomson Who proposed specific energy levels or shells for electrons to be found? A – Niels Bohr What was the positive particle that Rutherford used to shoot through the gold foil? A – Alpha particle

The Atom A, B, and C are considered what? A – Subatomic particles Which letter refers to the electron of the atom? A – A What type of charge does B have? A - 0 B C

Which two subatomic particles are nearly equal in mass? A – Protons and neutrons (B and C) What subatomic particle determines what element you have? A - Protons B C

State the Symbol NO PERIODIC TABLES Gold A – Au Potassium A – K Strontium A – Sr Manganese A - Mn Silver A – Ag Mercury A – Hg Selenium A – Se Xeon A - Xe

State the Name NO PERIODIC TABLES Ne A – Neon W A – Tungsten Kr A – Krypton Fe A – Iron Ti A – Titanium Cs A – Cesium Mg A – Magnesium Be Beryllium

An element is found to be malleable and have a shiny luster An element is found to be malleable and have a shiny luster. It is considered a … A – metal A new element is found and it is solid, shiny, decent conductor of heat, and brittle. What type of element can this be considered? A - metalloid

What is meant by the term “ion charge”? A – the number of electrons an atom may gain or lose from other atoms. What particle has to be removed from an atom so that the atom becomes a positive ion? A – electrons What kind of ions do elements on the right side of the periodic table form? A - negative

What periodic family has a common ion charge of zero? A – Noble gases What kind of reactivity will these elements have? A – none, stable, non-reactive Which family will react more with water – Alkali metals or Alkaline earth metals? A – alkali metals

What is a valence electron? A – an electron found in a valence shell which is the outermost shell for atoms. Why is H listed in the same column as the metals Li, Na, and K even though H is a non-metal? A – it want to give away one electron; therefore, it has the same number of valence electrons as the alkali family.

Identify the following atoms: 2,8,3 A – Aluminum 2,8,4 A – Silicon 2,7 A – Fluorine 2,8 A – Neon

Atomic Numbers and Atomic Masses A – Platinum Atomic # = 72 A – Hafnium Atomic mass = 258 A – Mendelevium Atomic mass = 88 A - Radium # of e- = 31 A – Gallium # of e- = 63 A – Europium Atomic # = 18 A – Argon Atomic mass = 51 A - Vanadium

What is Ca2+? It’s an … A – Ion What is Cl? It’s an … A – Atom What do the red dots represent? A – Electrons

Is the picture to the right a ionic or covalent bond? A – covalent How do you know? A – The electrons are being shared. What atoms are represented here? A – Hydrogen

What is the structure on the right called? A – A crystal lattice What is the most common crystal lattice known? A – NaCl (salt) What type of bonding produces crystal lattices? A – Ionic bonding

How are ionic bonds produced? A – When a metal and non-metal combine. The metal gives the non-metal electrons, causing it to become positive. The non-metal becomes negative and the positive and negative charges attract. What is a chemical formula? A – The symbols that show the elements in a compound and their ratios (relative number of each element in the compound)

Ionic Bonds – State the Name Rubidium is mixed with bromine. A – rubidium bromide Sulphur is mixed with calcium. A – calcium sulphide Cesium is mixed with phosphorus. A – Cesium phosphide Oxygen is mixed with strontium. A – Strontium oxide

Ionic Bonds – State the Formula Lithium combines with fluorine. A – LiF Calcium combines with chlorine. A – CaCl2 Silver combines with oxygen. A – Ag2O Scandium combines with sulphur. A – Sc2S3

Ionic Bonds – State the Formula Oxygen combines with calcium. A – CaO Tungsten combines with nitrogen. A – WN2 Barium combines with sulphur. A – BaS Zinc combines with bromine. A – ZnBr2

Multivalent Ions Give three examples of multivalent ions. A – Titanium, vanadium, iron, manganese, cobalt, nickel, copper, gold, mercury, etc. What do we need to do when naming compounds that contain multivalent ions? A – Use Roman numerals to indicate the ion charge for the metal

Multivalent Ions – State the Formulas Copper (II) oxide A – CuO Nickel (III) chloride A – NiCl3 Cobalt (III) oxide A – Co2O3 Manganese (IV) sulphide A – MnS2

Multivalent Ions – State the Name CrCl3 A – Chromium (III) chloride PbO A – Lead (II) oxide SnS2 A – Tin (IV) sulphide NiF3 A – Nickel (III) fluoride

Polyatomic Ions Give three examples of polyatomic ions. How are polyatomic ions bonded? A – By covalent bonds Do polyatomic ions have an ion charge? A – Yes Can polyatomic ions be bonded to metals in an ionic bond? A - Yes

Polyatomic Ions – State the Formula Potassium permanganate A – KMnO4 Lithium dichromate A – Li2Cr2O7 Calcium hydroxide A – Ca(OH)2 Magnesium phosphate A – Mg3(PO4)2