ATHS CDU UNIT

Chemistry Informal Diagnostics

Grade Level: 9
Stream: ADV
The year 2023/2024
 9ADV
4.1 – Periodic table of elements

4.1.1 Recall the names and symbols of common elements and their corresponding atomic
numbers, the first 20 elements.

4.1.2 Recognize the organization of elements in periods and groups on the periodic table.

1. A vertical column in the periodic table is known as

A. group
B. row
C. line
D. circle

2. Use the below periodic table and answer the following questions.

An element that belongs to Group 10 ------------------

An element that belongs to Group 1 _________________

An element that belongs to Period 4 _________________

 An element in Period 3 and Group 16 _________________

An element in Period 2 and Group 18 -------------------

3. Describe the basic organizational feature of the periodic table of the elements.

4.1.3-Classify elements into metals, nonmetals, and metalloids based on their properties and position in
the periodic table.
7. Which of the following is a metalloid?
A. Al
B. Si
C. Na
D. Hg

Use the periodic table and answer the questions 7 and 8

4. Which region of the periodic table contains metals?

A. M ,N and P
B. N and O
C. O, and P
D. P only

5. Which of the above regions contain nonmetals and metalloid elements?

A. M

B. N

C. O

D. P
6. Identify each of the following as a metal, a nonmetal, or a metalloid.

Element Metal/Nonmetal/metalloid
oxygen
Barium
Germanium
Iron

4.1.4-Categorize elements into metals and nonmetals based on their physical and chemical
characteristics by a guided inquiry.
7. Most of the elements in groups 16 through 18 are classified as

A. metalloids
B. Nonmetals
C. transition metals
D. metals
8. Describe the general characteristics of metals, nonmetals, and metalloids.

9. Xenon, a nonreactive gas used in strobe lights, is a poor conductor of heat and electricity. Would
you expect xenon to be a metal, a nonmetal, or a metalloid? Where would you expect it to be on the
periodic table? Explain.

10.4.1.5- Predict the properties of an element based on its position in the periodic table
14. Identify the following elements based on their position on the periodic table.
11. For each of the given elements, list two other elements with similar chemical properties.
a. iodine (I). ;
b. barium (Ba) ;
12. Give the chemical symbol for each element.
a. the element in period 3 that can be used in making computer chips because it is a metalloid
Si
b. the group 13, period 5 metal used in making flat screens for televisions
In
4.1.6-Analyze patterns in the periodic table to predict the reactivity and chemical behavior of
elements
Fill in the blanks

13. Metal reactivity decreases from left to right across periods and increases down groups.

14. Nonmetal reactivity increases from left to right and decreases down groups.
15. Which is the most reactive nonmetal?
A. Nitrogen
B. Chlorine
C. Fluorine
D. Bromine

16. Which is the most reactive metal

A. Calcium
B. Sodium
C. Rubidium
D. Cesium
17. Which property of an element can be predicted based on its position in the periodic table?
A. Atomic mass
B. Atomic number
C. Chemical reactivity
 D. Radioactivity
18. Which of the following elements will likely have similar chemical properties to `luorine?
A. Chlorine
B. Neon
C. Sodium
D. Magnesium

4.2-Quantum Theory and the Atom

4.2.1-Explain the principal energy levels and subshells in Bohr's model and their corresponding
quantum numbers.
19. In Bohr’s model of the atom, he proposed that electrons existed in orbits around the
nucleus. Each orbit was assigned a --------------to indicate its energy level.
A. quantum number
B. electron configuration
C. spin
D. s orbital
20. According to the quantum mechanical model of the atom, an orbital represents:
A. a position where an electron probably is
B. a position an electron must be
C. the point where an electron cannot be.
D. a surface beyond which electrons cannot go
21. What does n represent in the quantum mechanical model of the atom?

22. Compare and contrast Bohr’s model and the quantum mechanical model.

23 . Explain the relationship between energy levels and sublevels.

4.2.2- Understand the concept of an electron configuration diagram and its purpose in
representing the position of electrons in an atom's energy levels.
4.2.5 Differentiate between the shorthand notation and the diagrammatic representation of
electron configurations, using the correct format for writing the electron distribution.
4.2.6- Demonstrate the ability to draw accurate electron configuration diagrams for the first 20
elements on the periodic table
4.2.7-Explain the significance of electron configurations in determining an element's position on the
periodic table, including the number of shells and the number of electrons in the outermost shell.

24. Which element is represented by the electron configuration 1s22s22p63s23p64s2?

A. Boron
B. Calcium
C. Oxygen
D. Sodium

25. Which group is composed entirely of nonmetals?

A. 13

B. 14

C. 15

D. 18

26. The noble gas notation for magnesium is________.

A. [Ne]3s2
B. [Ne]2p63s2
C. [Ne]2s22p63s2
D. [Ne]1s22s22p63s2

27. Which of the following orbital notations is correct?

A. □_ □
1s 2s

B. □ □ □ __ __
1s 2s 2p
 C. □_ □ □ _ □_ □_ □ _
1s 2s 2p 3s
D. □ □ □ □ □ □_
1s 2s 2p 3s

28. Which of the following is/are NOT correct electron configuration(s)?

I. 1s2 2s12p2
II. 1s1 2s2 2p3 3p4
III. 1s2 2s2 3s2 4s2 2p63p6

A. I only
B. I and II only
C. I and III only
D. I, II and III

29. What can you conclude from the figure shown below?
A. Hund's rule has been violated.
B. The Aufbau principle has been violated
C. The Pauli exclusion principle has been violated.
D. This is a valid orbital diagram.

30. Which of the following is/are violated in the below orbital notation?

I. Hund’s Rule
II. Aufbau Principle
III. Pauli Exclusion principle

A. I only
B. II only
C. III only
D. I and II only

31. What can you conclude from the figure shown below?
 A. The Aufbau principle has been violated.
B. Hund's rule has been violated.
C. The Pauli exclusion principle has been violated.
D. This is a valid orbital diagram

32. What is the group and period, of an atom with the electron configuration [Ne]3s2,3p4

A. group 14, period 4,

B. group 16, period 3,

C. group 14, period 4,

D. group 16, period 4

33. Elements in the same group of the periodic table have the same

A. number of valence electrons

B. physical properties

C. number of electrons

D. electron configuration

34. In writing electron con`iguration, we follow certain rules. Match the Au`bau principle Pauli
Exclusion principle and Hund's rule with their correct statements by writing the letter of the
statement in front of the rule.

Hund's rule A Each electron occupies the lowest energy orbital

available
Pauli exclusion B maximum of two electrons can occupy a single atomic
principle orbital, but only if the electrons have opposite spins
C Single electrons with the same spin must occupy each
Aufbau principle equal-energy orbital before additional electrons with
opposite spins can occupy the same orbitals
35. Write the electron configuration and Noble gas configuration for the following elements.
Element Electron configuration Noble gas notation 36. Draw the orbital notation for
Li argon.

Na

Mg

Ca

19. What element is represented by each electron configuration?

a. [He]2s 2 2p 5 -

b. [Ar]4s2 -

c. [He]2s2-

37. Write the electron configuration and noble gas notation for the following elements.

Element Electron configuration Noble gas notation

38.Complete the missing parts in the table below.

Name of Element Symbol Electron configuration Number of valence electrons

1s22s22p63s23p6
 [Ne] 3s23p5

□ □ □_ ___ ___
1s 2s 2p

39. Explain how an atom’s valence electron configuration determines its place on the periodic
table.

40. The metal used to make soda cans has the electron configuration [Ne]3s2 3p1. Identify the metal and
give its group, period, and block in the periodic table.
Use the diagram to answer questions 24-27

41. Which shows the configuration of a nitrogen atom?

A. A
B. B
C. C
D. D
42. Which shows the configuration of a beryllium atom?
A. A
B. B
C. C
D. D

43. Which shows an orbital diagram that violates the Aufbau principle?
A. A
B. B
C. C
D. D
44. Which shows the configuration of a helium atom?
 A. A
B. B
C. C
D. D

44. Without using the periodic table, determine the group, period, and block of an atom with the
following electron configurations.

a. [Ne]3s2 b. [He]2s2, 2p3 c. [Ne]3s2 3p5

Electron configuration Group Period Valence

electron

[Ne]3s2

[He]2s2, 2p3

[Ne]3s2 3p5

45. Write the electron configuration of the following elements.

a. the group 2 element in the fourth period

b. the group 13 element in the 3rd period

c. the noble gas in the 3rd period

d. the group 16 element in the second period

4.2.3-Identify the key components of the Bohr model of the atom, including energy levels (shells),
electrons, and the nucleus.
46. What is/are the circular paths around the nucleus where electrons move in the Bohr model
called?
A. Neutron paths
 B. Proton paths
C. Rings
D. Shells or energy levels
47. What happens to an electron in the Bohr model when it absorbs energy, and how does this
relate to the energy levels (shells)?

48. Briefly discuss the concept of energy levels (shells) in the Bohr model and their significance in
understanding the arrangement of electrons in an atom

49. Describe the role of the nucleus in the Bohr model.

4.2.4 Apply the rules of the Bohr model to determine the maximum number of electrons that can occupy
each energy level.

50. How many orbitals are there in the energy level n?

A. n2
B. n
C. 2n2
D. 4n2

51. How many electrons can fit in the energy level n?

A. n2
B. n
C. 2n2
 D. 4n2

52. What is the maximum number of electrons that the fourth energy level can hold?
A. 8
B. 16
C. 18
D. 32

53. What is the maximum number of electrons that sublevel s can hold?
A. 2
B. 6
C. 10
D. 14

54. What is the maximum number of electrons that sublevel p can hold?
A. 2
B. 5
C. 6
D. 14

55. The sublevel(s) that make up the fourth energy level is/are ______.
A. S only
B. s and p only

C. s, p and d only

D. s, p, d and f

56. What is the maximum theoretical number of electrons related to the fifth principal energy level
of an atom?
A. 10
B. 20
C. 32
D. 50

57. Complete the table

 Principal Type of Number Number
quantum orbitals of of
number orbitals electrons
(n) (n2) (2n2)
1
s, p
3 9
4 32

4.3 Simple chemical formulas between metals & non-metals

4.3.1-Explore the meaning of valence electrons in the outermost energy level for common metals
and non-metals.

58. What are valence electrons?

A. Electrons in the innermost energy level

B. Electrons in the outermost energy level
C. Electrons in the nucleus
D. Protons in the outer shell

59. How does the number of valence electrons relate to the group number of an element in the
periodic table?
A. It is equal to the group number
B. It is half of the group number
C. It is unrelated to the group number
D. It is twice the group number

60. Elements in the same group have the same

A. atomic radius.
B. energy level of outer electrons.
C. number of valence electrons.
D. nuclear charge.
61. Why do elements within a group have similar chemical properties?

62. Do the atoms of Na and Mg have the same number of valence electrons?

63. De`ine valence electrons and explain their importance in the chemical behavior of an atom.

64. For a metal, describe the location of its valence electrons and how this in`luences its reactivity.

65. Explain the relationship between the number of valence electrons and the group number of an
element in the periodic table. Provide examples.

4.3.2-Explain how the transfer of electrons between metals and non-metals occurs to form ionic
compounds

66. Metals tend to __________ electrons and nonmetals tend to __________ electrons.
A. gain, gain
B. lose, lose
C. lose, gain
D. gain, gain
67. In the formation of ionic compounds, what generally happens to electrons?
A. They are shared
B. They are transferred
C. They are destroyed
D. They remain stationary
68. Which type of elements typically donate electrons to form positive ions in ionic compounds?
A. Metals
B. Non-metals
C. Metalloids
D. Noble gases

69. What force holds the oppositely charged ions together in an ionic compound?
a. Covalent bonding
b. Van der Waals forces
c. Ionic bonding
d. Metallic bonding

4.3.3 Analyze the electron configurations of metals and non-metals to understand their tendency
to lose or gain electrons in chemical reactions.

70. M is a __________, and N is a _________.

A. metal metal
B. metal non-metal
C. non-metal metal
D. non-metal non-metal

71. Which of the following electron configurations corresponds to non-metal?

I. 1s2 2s2 2p6 3s2

II. 1s2 2s22p6 3s2 3p5
III. 1s2 2s2 2p6 3s2 3p64s2 3d2

A. I only
B. II only
C. III only
D. I and III only
72. The noble gas notation of chlorine atom is _____________.

A. [Ar] 3s2 3p4

B. [Ar] 3s2 3p5
C. [Ne] 3s2 3p4
D. [Ne] 3s2 3p5

73. Which of the following elements is likely to have an electron conKiguration that
involves gaining electrons in chemical reactions?
a. Sodium (Na)
b. Chlorine (Cl)
c. Aluminum (Al)
d. Calcium (Ca)
74. What is the general trend in electron con`iguration for non-metals?
a. They gain electrons to achieve stability
b. They have full outer electron shells
c. They lose electrons to achieve stability
d. They share electrons with other elements
Consider the diagram below for the three different atoms M, R, and Q to answer questions 18
and19

75. Which of the atoms (M, R, or Q) can form a positive ion? Explain your answer.

76. Identify the atoms (M, R or Q) that can form a negative ion. Explain your answer.

4.3.4 Write formulas for simple ionic compounds using the charges of the ions and the principle of
electrical neutrality
4.3.5 Design and predict the chemical formulas of simple ionic compounds formed between metals
and non-metals using their respective charges and valence electrons (Examples: NaCl, MgBr2, CaO,
Al2O3)
77 What are the two different ions present in the compound AlP

A. Al3+, P3-
B. Al+,P2-
C. Al3+, P-
D. Al2+, P3-
78. Which substance is an ionic compound?
A. SrI2
B. N2O4
C. He
D. CCl4
79. Name the compound CaCl2
A. Calcium chloride
B. Carbon Chlorine
C. Chlorine calcium
D. Calcium carbide

80. Calcium bromide is the product of calcium and bromide ions. What is the formula
for calcium bromide?
A. CaBr
B. CaBr2
C. Ca2Br
D. Ca2Br2

81. Write the name and formula of the ionic compounds.

 NaCl, sodium oxide

KBr, cadmium sulfide

CaI2, magnesium nitride.

CsF, calcium phosphide.

LiCl, aluminum oxide

82. Explain why sodium oxide is a neutral compound.

4.3.4 Investigate the role of electrostatic attraction between oppositely charged ions in forming ionic

compounds in terms of melting point and physical properties.

83. How does the strength of electrostatic attraction between ions in an ionic compound relate to
its melting point?
a. Higher electrostatic attraction, higher melting point
b. Lower electrostatic attraction, higher melting point
c. Higher electrostatic attraction, lower melting point
d. No correlation between electrostatic attraction and melting point
84. Which physical property is often associated with ionic compounds due to their strong
electrostatic forces?
a. Low electrical conductivity
\b. Low solubility in water
c. High melting and boiling points
d. Low hardness

85. Which of the following statements is true regarding the physical properties of ionic
compounds?
a. They have low melting points and are poor conductors of electricity
b. They have high melting points and are good conductors of electricity
c. They have low melting points and are good conductors of electricity
d. They have high melting points and are poor conductors of electricity

86. Which of the following statements correctly describes (s) an ionic bond?

I. Involves metals and non-metals

II. Results from sharing electrons between the bonded atoms
III.Atoms bonded by ionic bonds attain the noble gas conAiguration of the nearest noble gas

A. I only
B. I and II only
C. I and III only
D. I, II, and III
87. Ahmed is testing the conductivity of ionic compound X using the equipment below. What
would Ahmed see in both a and b when he turns the switch on? Explain your answer.

88. List the physical properties of ionic compounds

5.1– Ionic vs Covalent Bonding; Ionic Compounds & Metals

5.1.3-Differentiate, using examples, empirical, molecular, and structural formulas

89. Which type of formula represents the simplest ratio of elements in a compound?
a. Molecular formula
b. Empirical formula
c. Structural formula
d. Isomeric formula

90. What type of formula provides information about the actual number and types of atoms in a
molecule?
a. Empirical formula
b. Molecular formula
c. Structural formula
d. Condensed formula
91. In the empirical formula for glucose (C6H12O6), what is the simplest ratio of carbon (C),
hydrogen (H), and oxygen (O) atoms?
a. 1:2:1
b. 2:1:1
c. 1:1:1
d. 3:2:1
92. Which type of formula uses lines to represent chemical bonds and shows the arrangement of
atoms in a molecule?
a. Molecular formula
b. Empirical formula
c. Structural formula
d. Condensed formula
93. If the molecular formula of a compound is C4H8, what is its empirical formula?
a. CH2
b. C2H4
c. CH
 d. C4H8
94. How do you distinguish between empirical molecular, and structural formulas of C2H6, CH4 ?

Molecular formula Empirical Structural Formula

Formula

5.1.4-Recognize and understand, using different examples, the differences between ball‐and‐stick models
and space‐filling models

95. How do you distinguish the differences between ball‐and‐stick models and space‐filling models

5.1.5-Differentiate, using examples, between atomic and molecular elements, ( Ca vs H2), and ionic and
molecular compounds (Ex: NaCl vs H2O)

96. Classify each compound as ionic or molecular.

a. CO2 -
b. NiCl2

c. NaI

d. PCl3.

97. Classify each element as atomic or molecular.

Ne;
F2;
K;
N2;

5.1.6-Explain the formation of metallic bonds through the "Sea Of Electrons" Model

98. A metallic bond is the attraction between the _________.

A. nucleus of the atom to its electrons

B. metal anion and the delocalized electrons

C. metal cation with the delocalized electrons

D. metal cation with the metal anions

99. Which of the following is/are the physical property(ies) of metals?
I. Ductile
II. Malleable
III. Good conductors of heat
A. I only
B. II only
C. I and II only
D. I, II and III

100. Explain the concept of the "Sea of Electrons" model in the formation of metallic bonds.

101. Use bonding in metals to explain the following properties.

 a) Metals are good conductors of heat and electricity.

b) Metals are malleable and ductile.

102. A student carries out a test to find the melting points of a range of substances. Their results
were:
Which substance is most likely to be a metal and why?

103 Explain bonding in a piece of aluminum.