Quizzes about: Atomic Radius ,Ionic Radii and Effective Nuclear Charge
Table of Contents
Atomic Radius ,Ionic Radii and Effective Nuclear Charge
Explore the concepts of atomic and ionic radii, effective nuclear charge, and size variations of ions in chemistry. Learn how these factors impact the properties of elements and compounds
Quiz1:Ionic Radii and Effective Nuclear Charge
Quiz2: Ionic Radii and Effective Nuclear Charge (Advanced)
Quiz3Ionic Radii and Effective Nuclear Charge (Advanced)
Quiz4 Test: Ionic Radii, Effective Nuclear Charge, and Related Concepts (Advanced)
Quiz 5: Graduation of Representative Elements and Atomic Radius
Quiz 6 : Estimating Ionic Bond Length
Quiz 7: Effective Nuclear Charge Concept
Quiz 8: Graduation of Atomic Radius, Atom-Ion Size Relation
Quiz1: Ionic Radii and Effective Nuclear Charge
1-True or False: Anions formed from nonmetal atoms are generally smaller in size compared to their neutral parent atoms.
2-Which of the following ions has the largest ionic radius?
a) Sodium ion (Na⁺)
b) Magnesium ion (Mg²⁺)
c) Potassium ion (K⁺)
d) Aluminum ion (Al³⁺)
3-True or False: As you move down a group (column) in the periodic table, metal atoms tend to form smaller cations.
4-The effective nuclear charge experienced by an ion is influenced by:
a) The nuclear charge and the number of protons in the nucleus.
b) The number of electrons and the number of neutrons.
c) The number of energy levels (shells) in the atom. d) The number of valence electrons.
5-Which of the following ions has the smallest ionic radius?
- a) Chloride ion (Cl⁻) b) Sulfate ion (SO₄²⁻) c) Nitride ion (N³⁻) d) Oxide ion (O²⁻)
6-True or False: The ionic radius of an anion is generally smaller than the atomic radius of its parent neutral atom.
7-Which of the following ions has the highest effective nuclear charge?
a) Magnesium ion (Mg²⁺)
b) Sodium ion (Na⁺)
c) Potassium ion (K⁺)
d) Lithium ion (Li⁺)
8-In a chemical reaction, a neutral iron atom (Fe) loses three electrons to form the iron(III) ion (Fe³⁺). How does the ionic radius of the iron(III) ion compare to the atomic radius of the neutral iron atom?
9-True or False: The effective nuclear charge of an ion is solely determined by the number of electrons in the ion.
10-When a nonmetal atom gains electrons to form anions, what effect does this have on the ionic radius?
1-Answer: False
2-Answer: c) Potassium ion (K⁺)
3-Answer: False
4-Answer: a) The nuclear charge and the number of protons in the nucleus.
5- Answer: c) Nitride ion (N³⁻)
6-Answer: False
7-Answer: a) Magnesium ion (Mg²⁺)
8-Answer: The ionic radius of the iron(III) ion (Fe³⁺) is smaller than the atomic radius of the neutral iron atom (Fe).
9-Answer: False
10-Answer: The ionic radius increases because the added electrons lead to increased electron-electron repulsion and greater shielding, causing the electron cloud to expand.
Quiz2: Ionic Radii and Effective Nuclear Charge
1-True or False: The effective nuclear charge (Zeff) experienced by an ion is always equal to its nuclear charge (atomic number).
2-Which of the following elements, when forming anions, tends to exhibit the largest increase in ionic radius compared to its neutral atom?
a) Carbon
b) Nitrogen (N)
c) Oxygen (O)
d) Sulfur (S)
3-In a chemical reaction, a neutral nitrogen atom (N) gains three electrons to form the nitride ion (N³⁻). How does the ionic radius of the nitride ion compare to the atomic radius of the neutral nitrogen atom?
4-Which of the following elements is most likely to form the smallest cation when losing electrons?
a) Calcium (Ca)
b) Potassium (K)
c) Magnesium (Mg)
d) Sodium (Na)
5-True or False: The effective nuclear charge (Zeff) experienced by an ion is influenced only by the nuclear charge and not by the number of electrons or electron configuration.
6-In a chemical reaction, a neutral oxygen atom (O) gains two electrons to form the oxide ion (O²⁻). How does the ionic radius of the oxide ion compare to the atomic radius of the neutral oxygen atom?
7-Which of the following cations has the highest effective nuclear charge?
a) Iron(II) ion (Fe²⁺)
b) Aluminum ion (Al³⁺)
c) Copper(I) ion (Cu⁺)
d) Zinc ion (Zn²⁺)
8-True or False: In general, cations formed from metal atoms are larger in size compared to the neutral metal atoms.
9-When a nonmetal atom loses electrons to form cations, what effect does this have on the ionic radius?
10-Compare the ionic radius of the aluminum ion (Al³⁺) to that of the aluminum atom (Al). Which is larger, and why?
1-Answer: False
2-Answer: d) Sulfur (S)
3-Answer: The ionic radius of the nitride ion (N³⁻) is larger than the atomic radius of the neutral nitrogen atom (N).
4-Answer: d) Sodium (Na)
5-Answer: False
6-Answer: The ionic radius of the oxide ion (O²⁻) is larger than the atomic radius of the neutral oxygen atom (O).
7-Answer: b) Aluminum ion (Al³⁺)
8-Answer: False
9-Answer: The ionic radius decreases because the loss of electrons results in a higher effective nuclear charge, causing the remaining electrons to be pulled closer to the nucleus.
10-Answer: The ionic radius of the aluminum ion (Al³⁺) is smaller than the atomic radius of the neutral aluminum atom (Al) because the ion has a higher effective nuclear charge, which attracts the remaining electrons more strongly.
Quiz 3 : Ionic Radii and Effective Nuclear Charge
1-True or False: The effective nuclear charge (Zeff) experienced by an ion is the same for all ions of the same element.
2-Which of the following ions has the smallest ionic radius?
a) Chromium(III) ion (Cr³⁺)
b) Nickel(II) ion (Ni²⁺)
c) Cobalt(II) ion (Co²⁺)
d) Iron(III) ion (Fe³⁺)
3-When a metal atom loses electrons to form a cation, what happens to the effective nuclear charge (Zeff)?
4-True or False: Cations formed from transition metals are generally smaller in size compared to those formed from main-group metals.
5-In a chemical reaction, a neutral sulfur atom (S) gains two electrons to form the sulfide ion (S²⁻). How does the ionic radius of the sulfide ion compare to the atomic radius of the neutral sulfur atom?
6-Which of the following ions has the highest effective nuclear charge?
a) Copper(II) ion (Cu²⁺)
b) Silver(I) ion (Ag⁺)
c) Zinc ion (Zn²⁺)
d) Lead(II) ion (Pb²⁺)
7-True or False: In general, nonmetal anions are smaller in size than nonmetal cations.
8-When a nonmetal atom gains electrons to form anions, what effect does this have on the ionic radius?
9-Compare the ionic radius of the oxygen ion (O²⁻) to that of the oxygen atom (O). Which is larger, and why?
10-In a chemical reaction, a neutral calcium atom (Ca) loses two electrons to form the calcium ion (Ca²⁺). How does the ionic radius of the calcium ion compare to the atomic radius of the neutral calcium atom?
1-Answer: False
2-Answer: a) Chromium(III) ion (Cr³⁺)
3-Answer: The effective nuclear charge (Zeff) increases.
4-Answer: True
5-Answer: The ionic radius of the sulfide ion (S²⁻) is larger than the atomic radius of the neutral sulfur atom (S).
6-Answer: a) Copper(II) ion (Cu²⁺)
7-Answer: True
8-Answer: The ionic radius increases because the added electrons lead to increased electron-electron repulsion and greater shielding, causing the electron cloud to expand.
9-Answer: The ionic radius of the oxygen ion (O²⁻) is larger than the atomic radius of the neutral oxygen atom (O) because the ion has gained electrons, leading to increased electron-electron repulsion and a larger electron cloud.
10-Answer: The ionic radius of the calcium ion (Ca²⁺) is smaller than the atomic radius of the neutral calcium atom (Ca).
Quiz 4 : Ionic Radii, Effective Nuclear Charge, and Related Concepts
1-True or False: The effective nuclear charge (Zeff) experienced by an ion is solely determined by the number of protons in the nucleus.
2-Which of the following ions has the highest effective nuclear charge?
a) Aluminum ion (Al³⁺)
b) Sodium ion (Na⁺)
c) Magnesium ion (Mg²⁺)
d) Potassium ion (K⁺)
3-When a nonmetal atom gains electrons to form anions, how does the number of energy levels (shells) in the atom typically change?
4-True or False: The size of ions formed from nonmetals is influenced solely by the number of electrons in the ion.
5-In a chemical reaction, a neutral lithium atom (Li) loses one electron to form the lithium ion (Li⁺). How does the ionic radius of the lithium ion compare to the atomic radius of the neutral lithium atom?
6-Which of the following ions has the smallest ionic radius?
a) Nitride ion (N³⁻)
b) Oxide ion (O²⁻)
c) Fluoride ion (F⁻)
d) Sulfide ion (S²⁻)
7-True or False: The effective nuclear charge experienced by an ion remains constant across different ionic charge states of the same element.
8-When a metal atom loses electrons to form a cation, what happens to the electron-electron repulsion in the electron cloud?
9-Compare the ionic radius of the iron(II) ion (Fe²⁺) to that of the iron(III) ion (Fe³⁺). Which is larger, and why?
10-True or False: The ionic radius of an anion is always larger than the atomic radius of its parent neutral atom.
1-Answer: False
2-Answer: a) Aluminum ion (Al³⁺)
3-Answer: The number of energy levels increases due to the addition of electrons.
4-Answer: False
5-Answer: The ionic radius of the lithium ion (Li⁺) is smaller than the atomic radius of the neutral lithium atom (Li).
6-Answer: a) Nitride ion (N³⁻)
7-Answer: False
8-Answer: The electron-electron repulsion decreases, leading to a more compact electron cloud.
9-Answer: The ionic radius of the iron(II) ion (Fe²⁺) is larger than that of the iron(III) ion (Fe³⁺) because the former has a lower positive charge and a lower effective nuclear charge.
10-Answer: True
Quiz 5: Graduation of Representative Elements and Atomic Radius
1-What influences the atomic radius of an atom?
a) Number of protons
b) Number of energy levels, effective nuclear charge, and electron-electron repulsion
c) Number of neutrons
d) Number of electrons in the outermost levelHow does the atomic radius
2-change as you move from left to right across a period?
a) Increases
b) Decreases
c) Remains constant
d) No predictable trend
3-In ionic compounds, how does the size of cations compare to their parent atoms?
a) Cations are larger
b) Cations are smaller
c) Cations have the same size
d) It depends on the specific element
4-Why is it impossible to precisely measure the atomic radius directly?
a) Electrons have well-defined boundaries
b) Nuclei have varying sizes
c) Electrons are described by probability distributions
d) Atomic radius is constant for all elements
5-What is the relationship between covalent bond length and atomic radius?
a) Covalent bond length is always equal to the atomic radius
b) Covalent bond length is shorter than the atomic radius
c) Covalent bond length is longer than the atomic radius
d) No relationship between the two
6-How can the atomic radius be estimated from a covalent bond length?
a) Add half of the covalent bond length to half of the covalent radius
b) Subtract half of the covalent bond length from half of the covalent radius
c) Multiply the covalent bond length by the covalent radius
d) Divide the covalent bond length by the covalent radius
7-What is the formula for calculating the atomic radius using the covalent bond length?
a) Atomic radius (r) = covalent bond length
b) Atomic radius (r) = covalent bond length / 2
c) Atomic radius (r) = covalent bond length * 2
d) Atomic radius (r) = covalent bond length + covalent radius
8-Why do cations have a smaller size compared to their parent atoms in ionic compounds?
a) They gain electrons
b) They lose electrons
c) They have more energy levels
d) They have fewer protons
9-What does the atomic radius depend on?
a) Number of neutrons
b) Number of energy levels, effective nuclear charge, and electron-electron repulsion
c) Number of protons
d) Number of electrons in the innermost level
10-Which method is commonly used to estimate atomic radii based on the distance between two covalently bonded atoms?
a) Ionic Radius
b) Covalent Radii
c) Nuclear Radius
d) Electron Radius
Answers:
1-b) Number of energy levels, effective nuclear charge, and electron-electron repulsion
2-b) Decreases
3-b) Cations are smaller
4-c) Electrons are described by probability distributions
5-b) Covalent bond length is shorter than the atomic radius
6-b) Subtract half of the covalent bond length from half of the covalent radius
7-b) Atomic radius (r) = covalent bond length / 2
8-b) They lose electrons
9-b) Number of energy levels, effective nuclear charge, and electron-electron repulsion
10-b) Covalent Radii
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11-What happens to the atomic radius as you move down a group in the periodic table?
a) Increases
b) Decreases
c) Remains constant
d) Depends on the specific element
12-Define the term “ionic radius” and how it differs from the atomic radius.
a) Ionic radius is the distance between two covalently bonded atoms, and it is larger than the atomic radius.
b) Ionic radius is the size of an ion, and it can be the same as the atomic radius.
c) Ionic radius is the atomic radius of an ion, and it is different for cations and anions.
d) Ionic radius is a measure of the size of an atom, and it is smaller than the atomic radius.
13-Why do anions have a larger size compared to their parent atoms in ionic compounds?
a) They gain protons
b) They gain electrons
c) They lose protons
d) They lose electrons
14-Which factor contributes to the decrease in atomic radius as you move from left to right across a period?
a) Increase in the number of energy levels
b) Increase in the effective nuclear charge
c) Increase in electron-electron repulsion
d) Decrease in the number of protons
15-Can atomic radius be directly measured? Why or why not?
a) Yes, because it is a fixed value for all elements.
b) Yes, because the position of electrons is well-defined.
c) No, because electrons do not have well-defined boundaries.
d) No, because atomic radius is constant across all periods.
16-How does the atomic radius vary within a group in the periodic table?
a) It increases
b) It decreases
c) It remains constant
d) It varies randomly
17-What is the relationship between cations and atomic size in ionic compounds?
a) Cations are larger than their parent atoms.
b) Cations have the same size as their parent atoms.
c) Cations are smaller than their parent atoms.
d) Cations have a variable size in comparison to their parent atoms.
18-Explain why atomic radius cannot be precisely defined or physically measured.
a) Electrons move too fast to be measured accurately.
b) Electrons do not have distinct boundaries like solid objects.
c) Nuclei are too small to be measured precisely.
d) Atomic radius is constantly changing.
19-Which of the following methods is NOT used to estimate atomic radii?
a) Covalent Radii
b) Ionic Radius
c) Nuclear Radius
d) Van der Waals Radius
20-How is the atomic radius related to the number of energy levels in an atom?
a) Atomic radius increases with an increase in the number of energy levels.
b) Atomic radius decreases with an increase in the number of energy levels.
c) Atomic radius is not affected by the number of energy levels.
d) Atomic radius is inversely proportional to the number of energy levels.
Answers:
- a) Increases
12-c) Ionic radius is the atomic radius of an ion, and it is different for cations and anions.
13-b) They gain electrons
14-b) Increase in the effective nuclear charge
15-c) No, because electrons do not have well-defined boundaries.
16-c) It remains constant
17-c) Cations are smaller than their parent atoms.
18-b) Electrons do not have distinct boundaries like solid objects. c) Nuclear Radius
19-a) Atomic radius increases with an increase in the number of energy levels.
Quiz 6 : Estimating Ionic Bond Length
1-What is the estimated bond length between two ions in an ionic compound based on?
a) Atomic radius
b) Covalent radius
c) Sum of the ionic radii of the cation and anion
d) Effective nuclear charge
2-How is the estimated bond length calculated in an ionic compound?
a) Subtracting ionic radii
b) Multiplying ionic radii
c) Adding ionic radii
d) Dividing ionic radii
3-What does the estimated bond length represent?
a) Distance between the outermost electrons
b) Distance between the centers of the nuclei of two bonded ions
c) Sum of the covalent radii
d) Effective nuclear radius
4-Why does the estimated bond length in an ionic compound depend on the ionic radii of the cation and anion?
a) Because the sum of the ionic radii determines the ion charge
b) Because the bond length is equal to the ionic radius of the anion
c) Because the distance between the centers of the nuclei depends on the sizes of the ions
d) Because the bond length is constant for all ionic compounds
5-What does the ionic radius depend on?
a) Atomic number
b) Number of protons
c) Number of electrons gained or lost to form ions
d) Number of energy levels
6-How is the estimated bond length in an ionic compound affected by the ionic radii of the ions?
a) It is inversely proportional
b) It is directly proportional
c) It remains constant
d) It is not affected
7-Calculate the estimated bond length in KBr based on the provided ionic radii:
Ionic Radius of Potassium Ion (K⁺): Approximately 1.33 Å
Ionic Radius of Bromide Ion (Br⁻): Approximately 1.96 Å
Answers:
1-c) Sum of the ionic radii of the cation and anion
2-c) Adding ionic radii
3-b) Distance between the centers of the nuclei of two bonded ions
4-c) Because the distance between the centers of the nuclei depends on the sizes of the ions
5-c) Number of electrons gained or lost to form ions
6-b) It is directly proportional
7-Estimated Bond Length (KBr) = 1.33 Å + 1.96 Å = 3.29 Å
c) It indicates the strength of the ionic bond
Quiz 7: Effective Nuclear Charge Concept
1-What does the effective nuclear charge (Zeff) take into account?
a) Only the actual nuclear charge
b) Only the shielding effect
c) Both the actual nuclear charge and the shielding effect
d) Only the electron-electron repulsion
2-How does a greater effective nuclear charge affect the atomic radius?
a) Increases the atomic radius
b) Has no effect on the atomic radius
c) Leads to a smaller atomic radius
d) Causes electron repulsion
4-What does the actual nuclear charge (Z) represent?
a) Total number of electrons in an atom
b) Total number of protons in the nucleus
c) Total number of neutrons in the nucleus
d) Total number of energy levels in an atom
5-What is the shielding effect in an atom?
a) The attraction between the outer electrons and the nucleus
b) The repulsion between inner electrons and outer electrons
c) The counteraction of electron-electron repulsion by inner electrons
d) The repulsion between protons in the nucleus
6-How is effective nuclear charge (Zeff) calculated?
a) Zeff = Z + Shielding Effect
b) Zeff = Z – Shielding Effect
c) Zeff = Z * Shielding Effect
d) Zeff = Z / Shielding Effect
7-What does Zeff represent in the effective nuclear charge concept?
a) Total number of electrons in an atom
b) The net positive charge experienced by an outer electron
c) The repulsion between inner electrons
d) The total positive charge in the nucleus
8-How does Zeff change as you move across a period from left to right in the periodic table?
a) Decreases
b) Remains constant
c) Increases
d) Depends on the specific element
9-In period 2 of the periodic table, which element has the highest effective nuclear charge (Zeff)?
a) Carbon (C)
b) Oxygen (O)
c) Fluorine (F)
d) Neon (Ne)
10-What trend is observed in Zeff as you move down a group in the periodic table?
a) Increases
b) Remains constant
c) Decreases
d) Varies randomly
Answers:
1-c) Both the actual nuclear charge and the shielding effect
2-c) Leads to a smaller atomic radius
3-b) Total number of protons in the nucleus
4-c) The counteraction of electron-electron repulsion by inner electrons
5-b) Zeff = Z – Shielding Effect
6-b) The net positive charge experienced by an outer electron
7-c) Increases
9-d) Neon (Ne)
10-c) Decreases
11-Why is the effective nuclear charge concept important in explaining atomic and chemical properties?
a) It determines the number of electrons in an atom.
b) It influences the number of energy levels in an atom.
c) It affects ionization energy, electron affinity, and chemical reactivity.
d) It defines the mass of an atom.
12-What is the relationship between effective nuclear charge and atomic size?
a) Higher Zeff leads to a larger atomic size.
b) Higher Zeff leads to a smaller atomic size.
c) Zeff has no effect on atomic size.
d) Atomic size is inversely proportional to Zeff.
13-How does the effective nuclear charge change as you move from left to right across a period in the periodic table?
a) Increases
b) Remains constant
c) Decreases
d) Reaches a maximum and then decreases
14-Which factor contributes to the decrease in atomic size as you move across a period from left to right?
a) Increase in shielding effect
b) Increase in Zeff
c) Decrease in electron-electron repulsion
d) Increase in the number of energy levels
15-Explain the significance of the shielding effect in the effective nuclear charge concept.
a) It enhances the attraction between protons and electrons.
b) It counteracts the attraction between protons and electrons.
c) It increases electron-electron repulsion. d) It has no impact on atomic properties.
16-How does Zeff influence the ionization energy of an atom?
a) Higher Zeff leads to higher ionization energy.
b) Higher Zeff leads to lower ionization energy.
c) Zeff has no effect on ionization energy.
d) Ionization energy is directly proportional to the number of energy levels.
17-Which element in period 2 of the periodic table has the smallest atomic size?
a) Lithium (Li)
b) Boron (B)
c) Carbon (C)
d) Oxygen (O)
18-What does Zeff represent in the formula Zeff = Z – Shielding Effect?
a) The total number of protons
b) The net positive charge experienced by an electron
c) The total number of electrons
d) The total number of neutrons
19-How does Zeff change as you move down a group (column) in the periodic table?
a) Increases
b) Remains constant
c) Decreases
d) Varies unpredictably
20-Why do electrons in the same energy level (shell) experience similar Zeff values?
a) They have different shielding effects.
b) They have different actual nuclear charges.
c) They are located in different orbitals.
d) They are shielded by the same inner electrons.
Answers:
- c) It affects ionization energy, electron affinity, and chemical reactivity.
12-b) Higher Zeff leads to a smaller atomic size. 13-a) Increases 14-b) Increase in Zeff
15-b) It counteracts the attraction between protons and electrons.
16-a) Higher Zeff leads to higher ionization energy. 17-d) Oxygen (O)
18-b) The net positive charge experienced by an electron 19-c) Decreases
20-d) They are shielded by the same inner electrons.
Quiz 8: Graduation of Atomic Radius, Atom-Ion Size Relation
1-What happens to the atomic radius as you move from left to right across a period in the periodic table?
a) Increases
b) Remains constant
c) Decreases
d) Fluctuates randomly
2-Why does the atomic radius generally decrease across a period from left to right?
a) Increase in electron shielding
b) Decrease in effective nuclear charge
c) Increase in effective nuclear charge
d) Decrease in the number of protons
3-What is the main factor responsible for the increase in atomic radius down a group in the periodic table?
a) Increase in effective nuclear charge
b) Decrease in electron shielding
c) Addition of more energy levels (shells)
d) Decrease in the number of energy levels
4-How does the effective nuclear charge change as you move across a period from left to right?
a) Increases
b) Remains constant
c) Decreases
d) Varies unpredictably
5-Which of the following pairs of elements illustrates the trend of decreasing atomic radius across a period?
a) Li (Lithium) and Cs (Cesium)
b) C (Carbon) and Si (Silicon)
c) N (Nitrogen) and O (Oxygen)
d) F (Fluorine) and I (Iodine)
6-What is the general trend for atomic radius as you move down a group in the periodic table?
a) Increases
b) Remains constant
c) Decreases
d) Fluctuates randomly
7-What happens to the atomic radius when a metal atom loses one or more electrons to become a cation?
a) Increases
b) Remains constant
c) Decreases
d) Depends on the specific metal
8-Why does a cation become smaller in size compared to its parent neutral metal atom?
a) Increase in electron shielding
b) Decrease in effective nuclear charge
c) Increased electron-electron repulsion
d) Decrease in the number of protons
9-In the sodium (Na) example, what happens to the ionic radius when sodium loses one electron to form Na⁺?
a) Increases
b) Remains constant
c) Decreases
d) Becomes unpredictable
10-Which element in the given pairs is larger in size, and why?
a) N (Nitrogen) and F (Fluorine)
b) Ba (Barium) and Be (Beryllium)
c) Cl (Chlorine) and Br (Bromine)
d) Fe²⁺ and Fe³⁺ (Iron ions)
Answers:
1-c) Decreases
2-c) Increase in effective nuclear charge
3-c) Addition of more energy levels (shells)
4-a) Increases
5-d) F (Fluorine) and I (Iodine)
6-a) Increases
7-c) Decreases
8-b) Decrease in effective nuclear charge
9-c) Decreases
10-a) N (Nitrogen) and F (Fluorine) – N (Nitrogen) is larger due to being in a higher period.
b) Ba (Barium) and Be (Beryllium) – Ba (Barium) is larger due to being lower down in the same group.
c) Cl (Chlorine) and Br (Bromine) – Br (Bromine) is larger due to being lower down in the same group.
d) Fe²⁺ and Fe³⁺ (Iron ions) – Fe²⁺ is larger due to having one less positive charge.
11-What happens to the size of an anion compared to its parent neutral nonmetal atom?
a) Increases
b) Remains constant
c) Decreases
d) Depends on the specific nonmetal
12-In the example of chlorine (Cl) forming a chloride ion (Cl⁻), what happens to the ionic radius?
a) Increases
b) Remains constant
c) Decreases
d) Becomes unpredictable
13-How does the addition of electrons influence the atomic radius of an anion?
a) Increases due to increased electron-electron repulsion
b) Decreases due to increased electron-electron repulsion
c) Has no effect on atomic radius
d) Depends on the number of added electrons
14-When comparing the atomic radius of a neutral iron atom to the ionic radius of Fe²⁺, what trend is observed?
a) Atomic radius is larger than ionic radius
b) Atomic radius is smaller than ionic radius
c) Atomic radius is equal to ionic radius
d) Atomic and ionic radii are unrelated
15-In the relation between the radii of metal atoms and their ions, what is the reason for the size decrease in cations?
a) Increased electron-electron repulsion
b) Decreased electron shielding
c) Increased electron shielding
d) Increased proton-proton repulsion
16-Which statement accurately describes the trend in size between the neutral Cl (Chlorine) atom and the Cl⁻ (chloride ion)?
a) Cl⁻ is larger due to increased electron-electron repulsion.
b) Cl⁻ is smaller due to increased electron-electron repulsion.
c) Cl⁻ is smaller due to decreased electron-electron repulsion.
d) Cl⁻ is larger due to decreased electron-electron repulsion.
17-In the example of sodium (Na) forming Na⁺, how does the effective nuclear charge change?
a) Increases
b) Remains constant
c) Decreases
d) Becomes unpredictable
18-Why does the atomic radius of an anion increase compared to its parent neutral nonmetal atom?
a) Decreased electron-electron repulsion
b) Increased electron-electron repulsion
c) Increased proton-proton repulsion
d) Decreased proton-proton repulsion
19-What is the primary factor determining the size of a metal cation in comparison to its parent neutral metal atom?
a) Increased electron-electron repulsion
b) Increased proton-proton repulsion
c) Decreased electron-electron repulsion
d) Decreased proton-proton repulsion
20-How does the atomic radius of an anion compare to the atomic radius of its parent neutral nonmetal atom?
a) Anion is larger due to decreased electron-electron repulsion.
b) Anion is smaller due to decreased electron-electron repulsion.
c) Anion is smaller due to increased electron-electron repulsion.
d) Anion is larger due to increased electron-electron repulsion.
Answers:
- a) Increases
12-a) Increases
13-a) Increases due to increased electron-electron repulsion
14-b) Atomic radius is smaller than ionic radius
15-c) Increased electron shielding
16-a) Cl⁻ is larger due to increased electron-electron repulsion.
17-c) Decreases
18-a) Decreased electron-electron repulsion
19-c) Decreased electron-electron repulsion
20-a) Anion is larger due to decreased electron-electron repulsion.
21-What is the primary reason for the decrease in atomic radius as you move from left to right across a period?
a) Decrease in the number of energy levels
b) Increase in the number of protons
c) Increase in electron-electron repulsion
d) Increase in electron shielding
22-In the example of forming chloride ions from chlorine atoms, how does the electron-electron repulsion change?
a) Increases
b) Remains constant
c) Decreases
d) Becomes unpredictable
23-Why do nonmetals generally form anions during chemical reactions?
a) To increase electron-electron repulsion
b) To decrease proton-proton repulsion
c) To increase proton-electron attraction
d) To gain electrons and achieve a stable electron configuration
24-Which of the following elements is expected to have the smallest atomic radius?
a) Lithium (Li)
b) Sodium (Na)
c) Potassium (K)
d) Francium (Fr)
25-How does the addition of more energy levels (shells) influence the atomic radius of an element?
a) Increases the atomic radius
b) Decreases the atomic radius
c) Has no effect on atomic radius
d) Depends on the number of added energy levels
26-In the formation of cations, why does the effective nuclear charge increase?
a) Due to an increase in electron shielding
b) Due to a decrease in electron-electron repulsion
c) Due to a decrease in the number of protons
d) Due to a decrease in the number of energy levels
27-Among the given pairs, which illustrates the trend of increasing atomic radius?
a) O (Oxygen) and S (Sulfur)
b) F (Fluorine) and Cl (Chlorine)
c) Na (Sodium) and K (Potassium)
d) P (Phosphorus) and Si (Silicon)
28-How does the effective nuclear charge change as you move down a group in the periodic table?
a) Increases
b) Remains constant
c) Decreases
d) Varies unpredictably
29-In the relation between the radii of metal atoms and their ions, what is the role of electron-electron repulsion?
a) Increases electron-electron repulsion
b) Decreases electron-electron repulsion
c) Has no effect on electron-electron repulsion
d) Depends on the specific metal
30-Explain the relation between the atomic radius of an atom and the ionic radius of its corresponding cation.
a) Atomic radius is equal to cationic radius
b) Atomic radius is larger than cationic radius
c) Atomic radius is smaller than cationic radius
d) Atomic and cationic radii are unrelated
Answers:
- b) Increase in the number of protons
22-c) Decreases
23-d) To gain electrons and achieve a stable electron configuration
24-a) Lithium (Li)
25-a) Increases the atomic radius
26-b) Due to a decrease in electron-electron repulsion
27-c) Na (Sodium) and K (Potassium)
28-a) Increases
29-b) Decreases electron-electron repulsion
30-c) Atomic radius is smaller than cationic radius