1. Chemistry Unit Review Game

2. 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

3. 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

4. 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.

5. 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

6. 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

7. 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

8. 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

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

10. 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

11. 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

12. 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

13. 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.

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

15. 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

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

17. 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

18. 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

19. 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)

20. 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

21. 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

22. 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

23. 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

24. 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

25. 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

26. 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

27. 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