directions: please answer each fill in the blank with the best answer.
1. a cation is an ion with an overall ______________ charge.
2. cations are made when an atom ______________.
3. the size of a positive ion is always ______________ than the size of the neutral atom of the same element.
4. as the positive charge on an ion increases, the size of the atom will ______________.
5. an anion is an ion with an overall ______________ charge.
6. anions are made when at atom ______________.
7. the size of a negative ion is always ______________ than the size of the neutral atom of the same element.
8. as the negative charge on an ion increases, the size of the atom will ______________.
9. which element/ion has the biggest atomic/ionic size in each of the following pairs? please circle your answer.
a)
b) na or na⁺¹
c) s or s²⁻
d) o⁻¹ or o²⁻
e) al or al³⁺
f) cu⁺¹ or cu²⁺
10. ______________ is the tendency for the atoms of the element to attract electrons when they are chemically combined with another element.
11. as you move across a period from left to right the electronegativity of an element will ______________.
12. as you move down a group, the electronegativity of an element will ______________.
13. the elements in group ______________ do not have defined values for electronegativities.
14. the highest possible value for electronegativity is ______________.
15. pick the element with the higher electronegativity:
a) br or i
d) p or na
b) k or ca
c) li or cs

Question

directions: please answer each fill in the blank with the best answer.
1. a cation is an ion with an overall ______________ charge.
2. cations are made when an atom ______________.
3. the size of a positive ion is always ______________ than the size of the neutral atom of the same element.
4. as the positive charge on an ion increases, the size of the atom will ______________.
5. an anion is an ion with an overall ______________ charge.
6. anions are made when at atom ______________.
7. the size of a negative ion is always ______________ than the size of the neutral atom of the same element.
8. as the negative charge on an ion increases, the size of the atom will ______________.
9. which element/ion has the biggest atomic/ionic size in each of the following pairs? please circle your answer.
 a)
 b) na or na⁺¹
 c) s or s²⁻
 d) o⁻¹ or o²⁻
 e) al or al³⁺
 f) cu⁺¹ or cu²⁺
10. ______________ is the tendency for the atoms of the element to attract electrons when they are chemically combined with another element.
11. as you move across a period from left to right the electronegativity of an element will ______________.
12. as you move down a group, the electronegativity of an element will ______________.
13. the elements in group ______________ do not have defined values for electronegativities.
14. the highest possible value for electronegativity is ______________.
15. pick the element with the higher electronegativity:
 a) br or i
 d) p or na
 b) k or ca
 c) li or cs

Accepted Answer

### Question 1 # Brief Explanations: A cation is a positively charged ion, so it has an overall positive charge. # Answer: positive ### Question 2 # Brief Explanations: Cations are formed when an atom loses electrons (since losing electrons leads to a positive charge as there are more protons than electrons). # Answer: loses electrons ### Question 3 # Brief Explanations: When an atom forms a positive ion, it loses electrons (usually from the outermost shell). Removing the outermost shell or electrons from it makes the ion smaller than the neutral atom. For example, Na (neutral) has more electron shells/electrons than Na⁺. # Answer: smaller ### Question 4 # Brief Explanations: As the positive charge on an ion increases, it means more electrons are lost. Losing more electrons pulls the remaining electrons closer to the nucleus (due to increased effective nuclear charge), so the size decreases. For example, Al (neutral) > Al⁺ > Al²⁺ > Al³⁺ in size. # Answer: decrease ### Question 5 # Brief Explanations: An anion is a negatively charged ion, so it has an overall negative charge (because it gains electrons, leading to more electrons than protons). # Answer: negative ### Question 6 # Brief Explanations: Anions are formed when an atom gains electrons (gaining electrons adds to the electron cloud, resulting in a negative charge as electrons outnumber protons). # Answer: gains electrons ### Question 7 # Brief Explanations: When an atom forms a negative ion, it gains electrons. These added electrons go into the outermost shell (or add to the electron cloud), increasing the electron - electron repulsions and making the ion larger than the neutral atom. For example, Cl (neutral) is smaller than Cl⁻. # Answer: larger ### Question 8 # Brief Explanations: As the negative charge on an ion increases, it means more electrons are gained. Gaining more electrons increases the electron - electron repulsions in the electron cloud, causing the size of the ion (and the atom from which it's formed) to increase. For example, O (neutral) < O⁻ < O²⁻ in size. # Answer: increase ### Question 9 #### Part b # Brief Explanations: Na is a neutral atom, and Na⁺ is a cation formed by Na losing an electron. When Na loses an electron, it loses its outermost electron shell (or electrons from the outermost shell), so Na is larger than Na⁺. # Answer: Na #### Part c # Brief Explanations: S is a neutral atom, and S²⁻ is an anion formed by S gaining two electrons. Gaining electrons increases the electron - electron repulsions in the electron cloud, so S²⁻ is larger than S. # Answer: S²⁻ #### Part d # Brief Explanations: O⁻ has a - 1 charge (gained 1 electron), and O²⁻ has a - 2 charge (gained 2 electrons). As the negative charge increases, more electrons are added, increasing electron - electron repulsions. So O²⁻ is larger than O⁻. # Answer: O²⁻ #### Part e # Brief Explanations: Al is a neutral atom, and Al³⁺ is a cation formed by Al losing three electrons. Losing electrons makes the ion smaller, so Al (neutral) is larger than Al³⁺. # Answer: Al #### Part f # Brief Explanations: Cu⁺ has a + 1 charge (lost 1 electron), and Cu²⁺ has a + 2 charge (lost 2 electrons). As the positive charge increases, more electrons are lost, increasing the effective nuclear charge on the remaining electrons, so the size decreases. Thus, Cu⁺ is larger than Cu²⁺. # Answer: Cu⁺ ### Question 10 # Brief Explanations: Electronegativity is defined as the tendency of an atom of an element to attract electrons when it is chemically combined with another element. # Answer: Electronegativity ### Question 11 # Brief Explanations: As we move across a period from left to right, the number of protons in the nucleus increases (atomic number increases) while the shielding effect remains relatively constant. This increases the effective nuclear charge, making the atoms more likely to attract electrons. So electronegativity increases across a period from left to right. # Answer: increase ### Question 12 # Brief Explanations: As we move down a group, the number of electron shells increases. The outermost electrons are further from the nucleus, and the shielding effect of inner electrons increases. This decreases the effective nuclear charge on the outermost electrons, so the tendency to attract electrons (electronegativity) decreases as we move down a group. # Answer: decrease ### Question 13 # Brief Explanations: The elements in group 18 (noble gases) are very stable and have a full valence electron shell. They rarely form chemical bonds (and when they do, it's under special conditions), so they do not have defined values for electronegativity as they do not show a tendency to attract electrons in chemical bonds. # Answer: 18 ### Question 14 # Brief Explanations: On the Pauling scale of electronegativity, the highest possible value is 4.0, which is assigned to fluorine (F). # Answer: 4.0 (for fluorine) ### Question 15 #### Part a # Brief Explanations: Br and I are in the same group (group 17). As we move down a group, electronegativity decreases. Br is above I in the group, so Br has a higher electronegativity than I. # Answer: Br #### Part b # Brief Explanations: K and Ca are in the same period (period 4). As we move across a period from left to right, electronegativity increases. Ca is to the right of K, so Ca has a higher electronegativity than K. # Answer: Ca #### Part c # Brief Explanations: Li and Cs are in the same group (group 1). As we move down a group, electronegativity decreases. Li is above Cs in the group, so Li has a higher electronegativity than Cs. # Answer: Li #### Part d # Brief Explanations: P and Na are in the same period (period 3). As we move across a period from left to right, electronegativity increases. P is to the right of Na, so P has a higher electronegativity than Na. # Answer: P

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