An overview

1.                  You should know the meaning and recognize the following words:

a.                   matter

b.                  gas

c.                   liquid

d.                  solid

e.                   pure substance

f.                    mixture

g.                   elements

h.                   compounds

i.                     atoms

j.                    solutions

k.                  solvent

l.                     solute

m.                 homogeneous

n.                   heterogeneous

o.                  saturated

p.                  point of saturation

q.                  emulsion

r.                    suspension

s.                   colloid

t.                    metal

u.                   non-metal

v.                   metalloid

w.                 family

x.                   group

y.                   period

z.                   transition element

aa.               representative element

bb.              noble gas

cc.               lanthanides

dd.              actinides

ee.               solidification

ff.                  fusion

gg.               vaporization

hh.               condensation

ii.                   sublimation

jj.                  atomic number

kk.              atomic mass

ll.                   valence electrons

mm.           octet rule

nn.               cation

oo.              anion

pp.              polyatomic ions

qq.              isotope

rr.                 Law of conservation of matter

ss.                Law of conservation of energy

tt.                  Exothermic

uu.               Endothermic

vv.               hydrocarbon


2.                  Recognize the difference between a physical change and a chemical change

3.                  Understand the Bohr model as it relates to the structure of the atom (nucleus, protons, electrons, neutrons, energy levels)

4.                  Draw the Lewis structure

5.                  Assign oxidation numbers to atoms based on their location in the periodic table

6.                  Understand the difference between ionic and molecular compounds, ionic and covalent bonds

7.                  Nomenclature

8.                  Balancing equations

9.                  Types of reactions (single displacement, double displacement, synthesis, decomposition, combustion)

10.              Recognize a base or an acid, based on characteristics and pH

11.              Recognize what affects the rate of a reaction


Questions to work on:


1. Fill the blanks:

a. A compound is formed of two, or many ________________________


b. A mixture in which a solid is dissolved in a liquid is called a __________________


c. A substance that is dissolved by the solvent is called a _______________________.


d. A heterogeneous mixture in which a liquid is mixed with another liquid is called a __________.


e. A solution is a ____________________ mixture.


f. When we cannot dissolve anymore solute in a solution, we say the solution is ______________.


g. A type of element that is a good conductor of electricity __________________________.


h. A carbon atom has ______________ valence electrons.


i. Nitrogen is a (an) _________________________ element.


j. Argon is a _____________________.


k. Calcium is in period _____________________________.


l. Aluminum is in family (group) ______________________________


m. Fusion is an __________________________ reaction.


n. Condensation is an ______________________ reaction.


o. A base produces _______________________ ions in solution.


p. An acid produces _______________________ ions in solution.


q. When a base reacts with an acid, they produce a _____________ and ________________.


r. An acid has a pH ______________ 7.


s. An __________________ changes color when mixed with a base or an    acid.


t. A /an ___________________ bond is formed between two non‑metals.


u. A/an ____________________ compound has a high fusion point.


v. A _______________________ has properties of both metals and non‑metals.


w. A proton has a mass, of   and a charge of _________________________


x. A neutron has a mass of ______________ and a charge of ________________.


y. An electron has a mass of _____________ and a charge of ___________________.


z. The _____________ explains the stability of elements that possess 8 valence electrons.


aa. Two atoms of the same element, which have different masses, are _________________.



2. Are the following elements M(metals), NM(non‑metals), or D(metalloids)


a. Sc: _______________


b. Se: _______________


c. As: _______________


d. Ar: _______________


e. Au: _______________


3. What is the Bohr model for the element, potassium?



4. What is the name or the symbol for the following elements?


a. B: ____________________________


b. N: ____________________________


c. Magnesium: ____________________


d. Sodium: _______________________


e. K: ____________________________


f. Li: ____________________________


g.: Aluminum: _____________________



5. What is the Lewis structure for Silicon?



6. What is the element that is in period 2 and‑in family IVA?


7. If an element has a mass of 35 and its atomic number is 17:


            a. How many protons? _________


            b. How many neutrons? _________


            c. How many electrons?_________


            d. What is the element?__________


8. Why do the atomic masses of the periodic table have decimal values?



9. What are the ions formed by the following elements?


a. Nitrogen: ______________


b. Helium: _______________


c. Sodium: ________________


d. Barium: ________________


e. Chlorine: ________________


10. What is the definition of an Arrhenius acid?



11. Ca+2:

a. a cation or an anion? ________________


b. how many electrons does it have? _______________


c. how many protons does it have? __________________


d. how many neutrons does it have? _________________


12. Write the formulas/names of the following compounds:


            a. copper (I) nitrate: _____________________


            b. mercury (II) bromide: ____________________


            c. nickel (III) sulfide: _______________________


            d. calcium carbonate: _____________________


            e. magnesium iodide: ______________________


            f. N2O5: ___________________________________________________


            g. A12O3: ___________________________________________________


            h. FeC12: ____________________________________________________


            i. Li2SO4: ___________________________________________________


            j. NiPO4: _______________________________________________________


13.    a. Balance the following reactions.

b. Indicate what type of reaction it is.


A. ____ NaClO3(s) → ______NaCl(s) + ____O2(g)


B. Type __________________________


C. ______ H2SO4(aq) + ______A12O3 (s) + → _____A12(SO4)3(aq) + ____H2O(l)


D. Type ________________________


E.  _______ Zn(s) + _____ FeC12(aq) → _______ ZnCl2(aq) + _______ Fe(s)


F. Type: _________________________


14. Write the following reactions using the appropriate symbols and then balance the equation.


a.         copper (II) sulfate reacts with nickel solid to produce nickel(III) sulfate and copper solid.


b.         magnesium oxide reacts with carbon dioxide to produce magnesium carbonate.


15.        Write the complete balanced combustion reaction of ethane (C2H6)?


16.        a. What is the rate of a reaction?

b. Identify three factors that affect the rate of reaction.


17.    Give three evidences of a chemical change?


18,    A + B → C + D + heat

         A + B + heat → C + D

Which one of the reactions above is an endothermic reaction?


19. If a solution has more H+ than OH-, it is described, as: acidic, basic or neutral?


20. Use IUPAC rules to name or write the formula for each of the following compounds:


            1. N2O5 __________________________________


            2. Fe(NO3)3 ________________________________


            3. PbCO3 ________________________________


            4. K3N ________________________________


            5. Ca(OH)2 ________________________________


            6.NaH ________________________________


            7. CBr4 ________________________________


            8. SCl2 ________________________________


            9. MgSO4 ________________________________


            10. NH4F ________________________________


            11.calcium bromide __________________________


            12. iron(II) iodide ____________________________


            13.aluminum sulfide _____________________________


            14. sodium phosphate_____________________________


            15. potassium carbonate ____________________________


            16. sulfur trioxide ____________________________________


            17. tin(II) nitrate ________________________________________


            18. iodine triflouride  _____________________________________


            19. ammonium phosphate ___________________________________


            20. dinitrogen tetroxide _______________________________________