Science 10-Unit 1-Chemistry Review
Name: ______
Date Due: ______
1. When zinc metal is placed in a solution of hydrochloric acid, it fizzes producing hydrogen gas and zinc chloride.
a) The reactants are ______
b) The products are ______
c) A word equation is: ______
2. In the following table, name the 3 major particles in the atom, state where they are located (in the nucleus or on the outside) and their charge.
Particle / Location / Charge3. List the four main points in John Dalton’s atomic theory.
1. ______
2. ______
3. ______
4. ______
4. Isotopes of an element are two different forms which have the same number of ______
and ______, but with different numbers of ______.
5. The atomic ______ of an element is the average mass of the isotopes which occur in nature.
6. In a neutral atom, the number of electrons is always equal to the number of
______or the ______number.
7. According to the model of the atom proposed by Neils Bohr, electrons move around the atom in ______or ______. When one orbit is filled, the electrons start filling the ______orbit.
8. The first orbit holds ______electrons.
The second orbit holds ______electrons.
The third orbit holds ______electrons.
9. Give the total number of electrons and the number of electrons in each orbit for each of the following elements:
Element / Total # ofelectrons / Electrons
in Level 1 / Electrons
in Level 2 / Electrons
in Level 3 / Electrons
in Level 4
Aluminum (Al)
Nitrogen (N)
Calcium (Ca)
Lithium (Li)
Argon (Ar)
10. Draw the Bohr models for neutral atoms of each of the following elements.
a) oxygen
b) chlorine
c) phosphorus
d) magnesium
11. In order to have the same number of electrons as the noble gas neon, sodium
would have to ______electron.
gain/lose #
12. Name iodine Symbol ______Atomic number _____ # of electrons _____
In order to have the same number of electrons as the noble gas xenon, iodine
would have to ______electron. Is iodine a metal or non-metal?______
gain/lose #
13. Classify each of the following elements as an alkali metal, alkaline earth, halogen, noble gas or transition metal:
Element / FamilyFe
BrK
Kr
Ba
F
Pt
Li
Ne
Ra
14. Mendeleev arranged the elements in order of ______
and also put them in groups based on similar ______.
15. What did Mendeleev do when he came to a space where no known element would fit?
______
16. Vertical columns of the Periodic Table are known as Groups or Chemical ______.
17. Elements are no longer listed in order of atomic mass, but in order of atomic ______.
18. What is similar about elements in the same family? ______
19. What would alkali metal atoms need to do in order to end up with the same stable electron
arrangements as the noble gases? ______
20. The outer orbits of halogen atoms each have ______electrons. This is one
(more/less) ______than the nearest noble gas atom.
21. In order to achieve the stable arrangement of noble gas atoms, each halogen atom would
have to ______electron.
gain/lose #
22. Are the halogens metals or non-metals? ______
23. Fill in the following table:
Indicator / Colour in Acid / Colour in BaseRed Litmus
Blue Litmus
24. Are the pH’s of Acid Solutions < 7, >7 or = 7? ______
Are the pH’s of Base Solutions < 7, >7 or = 7? ______
25. The more acidic a solution is, the (lower/higher) the pH? ______
26. The more basic a solution is, the (lower/higher) the pH? ______
27. A solution with a pH = 7 is said to be ______
28. An acid HCl is mixed with a base KOH. Predict the chemical formulas for the two
products of this reaction. ______and ______. This
type of reaction of an acid reacting with a base is called ______
29. List 4 properties (characteristics) all acids have in common:
______
______
______
______
30. List 4 properties (characteristics) all bases have in common:
______
______
______
______
31. Which family of elements has just enough electrons in their valence energy levels to
completely fill them up? ______
32. If Lithium is combined with Fluorine, the Lithium atom will ______an
gain/lose
electron to the Fluorine atom.
33. When Fluorine has gained an electron, it now has ____ protons (remember, it doesn’t lose
any protons), and ____ electrons. Because protons are positive (+) and electrons are
negative (-), the charge left over is _____. The Fluorine is no longer a neutral atom, but
is a charged atom, which is called a Fluoride ______.
34. Because the lithium ion (Li+) and the fluoride ion (F-) have opposite charges, they
______each other. This attraction forms an ______
bond.
35. Generally, combining capacity means the number of ______an atom
needs to lose or gain in order to have the same number of electrons as a ______
______.
36. Use the Periodic Table and the method shown to you by the teacher to write the correct formulas for the following ionic compounds.
a) magnesium iodide ...... ______
b) aluminum fluoride ...... ______
c) calcium sulphide ...... ______
d) rubidium oxide ...... ______
e) sodium phosphide ...... ______
f) iron (III) sulphate ...... ______
g) manganese (IV) oxide ...... ______
h) copper (II) phosphate ...... ______
i) calcium nitrate ...... ______
j) ammonium chloride ...... ______
k) lithium oxalate ...... ______
l) nickel (III) carbonate ...... ______
m) copper (I) permanganate ...... ______
n) ammonium sulphate ...... ______
37. Compounds with only two elements are called ______compounds.
38. In a binary compound, the non-metal changes it’s name so it ends in the letters ______.
39. In a compound containing a polyatomic ion, the name of the polyatomic ion
(always/sometimes/never)______changes.
40. Write the correct names for the following ionic compounds Spelling counts!
a) Na3PO4 ...... ______
b) K2S ...... ______
c) Rb2SO3 ...... ______
d) (NH4)2CO3 ...... ______
e) Ba(OH)2 ...... ______
f) MgSO4 ...... ______
g) Cs2HPO4 ...... ______
h) NaHCO3 ...... ______
i) AgNO3 ...... ______
j) Na3As ...... ______
k) NH4NO3 ...... ______
l) Ag2Cr2O7 ...... ______
41. In an ionic compound, electrons are ______from one atom
to the other. The element that lost electron(s) becomes a (+/-) ______ion and the
element than gains electron(s) becomes a (+/-) ______ion. The two oppositely charged
ions now (attract/repel) ______each other.
42. In a covalent compound, one atom ______electrons with another atom.
43. Give the formulas for molecules of the seven diatomic elements. The first one is H2.
______
44. Write the correct formulas for the following MOLECULAR compounds:
a) nitrogen trioxide ...... ______
b) silicon tetrafluoride ...... ______
c) nitrogen monoxide ………………………… ______
d) selenium hexafluoride ...... ______
e) phosphorus pentachloride ...... ______
f) sulphur dioxide ...... ______
g) dinitrogen tetroxide ...... ______
45. Write the correct names for the following MOLECULAR compounds:
a) PF5 ...... ______
b) SO3 ...... ______
c) ClF6 ...... ______
d) SeO2...... ______
e) N2O ...... ______
f) N2Cl4 ...... ______
46. What is meant by a physical change?
47. What is meant by a chemical change?
48. Balance the following equations by putting the proper coefficients wherever they are
needed. Classify the reaction type.
a) strontium + oxygen à strontium oxide
b) aluminum + water à aluminum hydroxide + hydrogen
c) aluminum + oxygen à aluminum oxide
d) C5H12 + oxygen à
e) sodium + water à
f) NaClO3 à NaCl + O2
g) Ca(NO3)2 + (NH4)2SO4 à
h) C2H5OH + O2 à CO2 + H2O
i) Al(NO3)3 + K2CrO4 à
j) NH3 à N2 + H2
k) C6H6 + O2 à
l) sulfur + oxygen à sulfur dioxide
m) nitric acid + iron (III) hydroxide à
n) Br2 + CaCl2 à
49. Calculate the molar mass of the following compounds
a) H20
b) Aluminum chloride
c) K2Cr2O7
50. Convert the following masses to chemical amount (moles)
a) 5.0g of NaCl
b) 2.8g of copper(II)phosphate
51. Convert the following chemical amounts to masses
a) 3.14 moles of methane
b) 5.5 moles of H2SO4
Course Review – Unit 1 Chemistry Page 12