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Chemistry Unit Review Game. Chapter 1 Anything that has mass and volume is considered to be??? Anything that has mass and volume is considered to be???

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Presentation on theme: "Chemistry Unit Review Game. Chapter 1 Anything that has mass and volume is considered to be??? Anything that has mass and volume is considered to be???"— Presentation transcript:

1 Chemistry Unit Review Game

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

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

4 Dalton’s Atomic Theory – Main Points All matter is made of small particles called atoms. All matter is made of small particles called atoms. Atoms cannot be created, destroyed, or divided into smaller particles. 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. 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. Compounds are created when atoms of different elements link together in definite proportions.

5 Who proposed the “raisin bun” model of the atom? 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? 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? What was the positive particle that Rutherford used to shoot through the gold foil? A – Alpha particle

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

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

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

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

10 An element is found to be malleable and have a shiny luster. It is considered a … 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 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

11 What is meant by the term “ion charge”? 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? 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? What kind of ions do elements on the right side of the periodic table form? A - negative

12 What periodic family has a common ion charge of zero? What periodic family has a common ion charge of zero? A – Noble gases What kind of reactivity will these elements have? 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? Which family will react more with water – Alkali metals or Alkaline earth metals? A – alkali metals

13 What is a valence electron? 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? 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.

14 Identify the following atoms: Identify the following atoms: 1. 2,8,3 A – Aluminum 2. 2,8,4 A – Silicon 3. 2,7 A – Fluorine 4. 2,8 A – Neon

15 Atomic Numbers and Atomic Masses Atomic # = 78 Atomic # = 78 A – Platinum Atomic # = 72 Atomic # = 72 A – Hafnium Atomic mass = 258 Atomic mass = 258 A – Mendelevium Atomic mass = 88 Atomic mass = 88 A - Radium # of e- = 31 # of e- = 31 A – Gallium # of e- = 63 # of e- = 63 A – Europium Atomic # = 18 Atomic # = 18 A – Argon Atomic mass = 51 Atomic mass = 51 A - Vanadium

16 What is Ca 2+ ? It’s an … What is Ca 2+ ? It’s an … A – Ion What is Cl? It’s an … What is Cl? It’s an … A – Atom What do the red dots represent? What do the red dots represent? A – Electrons

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

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

19 How are ionic bonds produced? 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? 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)

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

21 Ionic Bonds – State the Formula Lithium combines with fluorine. Lithium combines with fluorine. A – LiF Calcium combines with chlorine. Calcium combines with chlorine. A – CaCl 2 Silver combines with oxygen. Silver combines with oxygen. A – Ag 2 O Scandium combines with sulphur. Scandium combines with sulphur. A – Sc 2 S 3

22 Ionic Bonds – State the Formula Oxygen combines with calcium. Oxygen combines with calcium. A – CaO Tungsten combines with nitrogen. Tungsten combines with nitrogen. A – WN 2 Barium combines with sulphur. Barium combines with sulphur. A – BaS Zinc combines with bromine. Zinc combines with bromine. A – ZnBr 2

23 Multivalent Ions Give three examples of 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? 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

24 Multivalent Ions – State the Formulas Copper (II) oxide Copper (II) oxide A – CuO Nickel (III) chloride Nickel (III) chloride A – NiCl 3 Cobalt (III) oxide Cobalt (III) oxide A – Co 2 O 3 Manganese (IV) sulphide Manganese (IV) sulphide A – MnS 2

25 Multivalent Ions – State the Name CrCl 3 CrCl 3 A – Chromium (III) chloride PbO PbO A – Lead (II) oxide SnS 2 SnS 2 A – Tin (IV) sulphide NiF 3 NiF 3 A – Nickel (III) fluoride

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

27 Polyatomic Ions – State the Formula Potassium permanganate Potassium permanganate A – KMnO 4 Lithium dichromate Lithium dichromate A – Li 2 Cr 2 O 7 Calcium hydroxide Calcium hydroxide A – Ca(OH) 2 Magnesium phosphate Magnesium phosphate A – Mg 3 (PO 4 ) 2


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