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Chemistry Test

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

1. 

Each inner energy level of an atom has maximum numbers of _____ it can hold.
a.
electrons
c.
quarks
b.
neutrons
d.
protons
 

2. 

Dot diagrams are used to represent _____.
a.
atomic numbers
b.
atomic mass
c.
isotopes
d.
outer electrons
e.
the structure of the nucleus
 

3. 

A chemical symbol represents the _____ of an element.
a.
name
b.
reaction
c.
group
d.
structure
e.
type
 

4. 

Horizontal rows of the periodic table are called _____.
a.
clusters
b.
families
c.
groups
d.
periods
e.
quarks
 

5. 

Atoms of the same element with different numbers of neutrons are called _____.
a.
isotopes
b.
metals
c.
metalloids
d.
radioactive
e.
transition elements
 

6. 

A particle that moves around the nucleus is _____.
a.
an electron
b.
an ion
c.
a neutron
d.
a quark
e.
a proton
 

7. 

Elements in Groups 3 through 12 of the periodic table are called _____.
a.
isotopes
b.
metalloids
c.
metals
d.
noble gases
e.
transition elements
 

8. 

A certain atom has 26 protons, 26 electrons, and 30 neutrons. Its mass number is _____.
a.
26
b.
30
c.
52
d.
56
e.
82
 

9. 

In a chemical formula, the ratio of atoms in the compound is shown by numbers called _____.
a.
hydrates
b.
chemical symbols
c.
oxidation numbers
d.
subscripts
e.
superscripts
 

10. 

A group of atoms that acts together as one charged atom is a _____.
a.
crystal
c.
negative ion
b.
molecule
d.
polyatomic ion
 

11. 

The elements that make up a compound and the ratios of the atoms of those elements can be shown in a _____.
a.
chemical formula
c.
subscript
b.
chemical symbol
d.
superscript
 

12. 

A chemical bond that occurs when atoms share electrons is _____ bond.
a.
a covalent
c.
a magnetic
b.
an ionic
d.
a polyatomic
 

13. 

The name given to the combining ability of an atom is _____.
a.
atomic mass
c.
ionic number
b.
atomic number
d.
oxidation number
 

14. 

The sum of the oxidation numbers in a neutral compound is _____.
a.
a negative number
c.
a positive number
b.
one
d.
zero
 

15. 

The oxidation number of an atom is shown with a _____.
a.
negative number
c.
subscript
b.
positive number
d.
superscript
 

16. 

How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable?
a.
2
b.
4
c.
6
d.
8
e.
10
 

17. 

What kind of chemical bond is formed when electrons are transferred from atom to atom?
a.
covalent
c.
ionic
b.
hydrate
d.
magnetic
 

18. 

What is the total number of atoms in the compound Ca(ClO3)2?
a.
2
b.
3
c.
5
d.
6
e.
9
 

19. 

How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2?
a.
3
b.
4
c.
7
d.
11
e.
12
 

20. 

What is the name of the compound with the formula NaCl?
a.
chlorine sodiate
c.
sodium chloride
b.
sodium chlorate
d.
sodium dichloride
 

21. 

Why do the noble gases NOT form compounds readily?
a.
They have empty outer energy levels.
b.
They have no electrons.
c.
They have seven electrons in the outer energy levels.
d.
Their outer energy levels are completely filled with electrons.
 

22. 

What is the ratio of potassium atoms to oxygen atoms in a binary compound made from these two elements?
a.
1:1
b.
1:2
c.
1:3
d.
2:1
e.
3:1
 

23. 

What is the name of a binary compound made up of lithium and chlorine?
a.
chlorine lithiate
c.
lithium chloride
b.
chlorine lithium
d.
lithium chlorate
 

24. 

Which of the following is the correct formula for magnesium nitrate?
a.
MgNO3
c.
Mg(NO3)2
b.
Mg2NO3
d.
Mg2(NO3)2
 

25. 

What is the charge of phosphate in K3PO4?
a.
7-
b.
3-
c.
1+
d.
5+
e.
4+
 

26. 

What is the correct formula for magnesium oxide?
a.
MgO
c.
Mg2O2
b.
MgO2
d.
Mg2O
 

27. 

At room temperature, most metals are _____.
a.
gases
c.
radioactive
b.
liquids
d.
solids
 

28. 

Hydrogen is grouped with the alkali metals because it _____.
a.
does not readily form compounds
c.
is a gas
b.
has one electron in its outer energy level
d.
is a metal
 

29. 

The elements in Groups 3-12 of the periodic table are the _____.
a.
actinides
b.
alkaline earth metals
c.
alkali metals
d.
halogens
e.
transition elements
 

30. 

A family of elements that has two electrons in its outer energy level is the _____.
a.
actinides
b.
alkaline earth metals
c.
alkali metals
d.
halogens
e.
transition elements
 

31. 

Bromine is the only halogen and nonmetal that is normally a _____.
a.
gas
c.
semiconductor
b.
liquid
d.
solid
 

32. 

The only metal that is a liquid at room temperature is _____.
a.
copper
b.
mercury
c.
silver
d.
sodium
e.
zinc
 

33. 

Three transition elements in Group 12 of the periodic table are _____.
a.
copper, silver, and gold
c.
mercury, zinc, and cadmium
b.
iron, nickel, and cobalt
d.
neon, helium, and xenon
 

34. 

The only noble gas with fewer than eight electrons in its outer level is _____.
a.
helium
c.
radium
b.
neon
d.
xenon
 

35. 

Elements that lie along the stair-step line of the periodic table are _____.
a.
liquids
c.
metalloids
b.
metals
d.
radioactive
 

36. 

A family of elements that contains the most reactive metals is the _____.
a.
actinides
b.
alkaline earth metals
c.
alkali metals
d.
transition elements
e.
noble gases
 

37. 

When one element displaces another element in a compound, the reaction is a _____ reaction.
a.
decomposition
c.
single-displacement
b.
double-displacement
d.
synthesis
 

38. 

Each substance to the right of the arrow in a chemical equation is a(n) _____.
a.
catalyst
b.
inhibitor
c.
precipitate
d.
product
e.
reactant
 

39. 

A chemical reaction in which energy is released is _____.
a.
endothermic
b.
exothermic
c.
flammable
d.
a formula
e.
an inhibitor
 

40. 

Numbers that precede symbols and formulas in a chemical equation are _____.
a.
catalysts
b.
coefficients
c.
fractions
d.
subscripts
e.
superscripts
 

41. 

A term that means "putting together" is _____.
a.
catalyst
b.
decomposition
c.
product
d.
reactant
e.
synthesis
 

42. 

The breaking down of a compound into simpler substances is _____.
a.
decomposition
c.
product
b.
displacement
d.
synthesis
 

43. 

Each substance on the left side of the arrow in a chemical equation is a _____.
a.
catalyst
b.
coefficient
c.
product
d.
reactant
e.
synthesis
 

44. 

In a chemical equation, the symbol that means "dissolved in water" is _____.
a.
(aq)
b.
(cr)
c.
(dw)
d.
(I)
e.
(g)
 

45. 

Which of the following is a balanced chemical equation?
a.
AgNO3 + NaCl —> 4AgCl + 2NaNO3
c.
AgNO3 + NaCl —> AgCl + NaNO3
b.
2AgNO3 + 2NaCl —> 3AgCl + 2NaNO3
d.
AgNO3 + 2NaCl —> AgCl + 3NaNO3
 

46. 

_____ chemical equation has the same number of atoms of each element on each side of the equation.
a.
A balanced
c.
A simple
b.
A complex
d.
An unbalanced
 

47. 

What type of reaction is shown in the following chemical equation? NH3 + HCl —> NH4Cl
a.
decomposition
c.
single displacement
b.
double displacement
d.
synthesis
 

48. 

According to the law of conservation of mass, how does the mass of the products in a chemical reaction compare to the mass of the reactants?
a.
There is no relationship.
c.
The mass of the reactants is greater.
b.
The mass of the products is greater.
d.
The masses are equal.
 

49. 

What type of reaction is shown in the following chemical equation? 2H2O —> 2H2 + O2
a.
decomposition
c.
single displacement
b.
double displacement
d.
synthesis
 

50. 

What is an insoluble solid that forms as the result of a chemical reaction?
a.
an aqueous
c.
an inhibitor
b.
a catalyst
d.
a precipitate
 

Matching
 
 
chemistry_retake_files/i0530000.jpg

Match each of the models in Figure 16-1 with the type of reaction it represents.
a.
single displacement
b.
decomposition
c.
double displacement
d.
synthesis
 

51. 

Model 1
 

52. 

Model 2
 

53. 

Model 3
 

54. 

Model 4
 



 
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