Question

a. circle the element with the lower reactivity:

1. nitrogen or fluorine 2. tellurium or sulfur
2. aluminum or magnesium 4. chlorine or iodine

b. circle the element with the lowest reactivity:

1. boron or neon 2. radon or krypton
2. bromine or arsenic 4. phosphorus or aluminum

c. circle the element with the higher reactivity:

1. phosphorus or chlorine 2. strontium or magnesium
2. scandium or potassium 4. bromine or fluorine

d. circle the element with the higher reactivity:

1. calcium or barium 2. silicon or chlorine
2. selenium or oxygen 4. cesium or sodium

e. circle the element that is more reactive, and box the element that has the lowest electronegativity.
s cl se br
f. circle the element that is least reactive.
n o p s
g. circle the element that is more reactive.
na mg k ca
h. circle the element that is more reactive.
be li na mg

Explanation:

• A1: Nitrogen has lower reactivity than Fluorine. Fluorine is highly reactive as it is a halogen and needs only one electron to complete its octet. Nitrogen has a stable triple - bond in its diatomic form (\(N_2\)) and is less reactive.
• A2: Tellurium is less reactive than Sulfur. In group 16 (chalcogens), reactivity decreases down the group. Sulfur is above Tellurium in the group.
• A3: Aluminum is less reactive than Magnesium. Magnesium is more electropositive (loses electrons more easily) than Aluminum.
• A4: Iodine is less reactive than Chlorine. In group 17 (halogens), reactivity decreases down the group. Chlorine is above Iodine in the group.
• B1: Neon is less reactive than Boron. Neon is a noble gas with a complete octet, while Boron is a metalloid and can form compounds.
• B2: Krypton is less reactive than Radon. Noble gas reactivity (though very low in general) increases slightly down the group, and Krypton is above Radon.
• B3: Arsenic is less reactive than Bromine. Bromine is a halogen (more reactive non - metal) and Arsenic is a metalloid.
• B4: Aluminum is less reactive than Phosphorus. Phosphorus can form various compounds more readily than Aluminum in some common reactions.
• C1: Chlorine is more reactive than Phosphorus. Chlorine is a highly reactive halogen.
• C2: Strontium is more reactive than Magnesium. In group 2 (alkaline earth metals), reactivity increases down the group. Strontium is below Magnesium.
• C3: Potassium is more reactive than Scandium. Potassium is an alkali metal (highly reactive, loses one electron easily) and Scandium is a transition metal.
• C4: Fluorine is more reactive than Bromine. In group 17, reactivity decreases down the group, and Fluorine is above Bromine.
• D1: Barium is more reactive than Calcium. In group 2, reactivity increases down the group. Barium is below Calcium.
• D2: Chlorine is more reactive than Silicon. Chlorine is a halogen (reactive non - metal), Silicon is a metalloid.
• D3: Oxygen is more reactive than Selenium. In group 16, reactivity decreases down the group. Oxygen is above Selenium.
• D4: Cesium is more reactive than Sodium. In group 1 (alkali metals), reactivity increases down the group. Cesium is below Sodium.
• E:
• More reactive: Chlorine (\(Cl\)) is more reactive among \(S\), \(Cl\), \(Se\), \(Br\) as it is a halogen and more electronegative.
• Lowest electronegativity: Selenium (\(Se\)) has the lowest electronegativity. Electronegativity decreases down a group (for non - metals in the same group) and Selenium is below Sulfur and Chlorine (in terms of position in relevant groups).
• F: Nitrogen (\(N\)) is the least reactive among \(N\), \(O\), \(P\), \(S\). Oxygen is a reactive non - metal, Phosphorus and Sulfur can form various compounds more readily in many common reactions compared to Nitrogen (due to its stable \(N_2\) form).
• G: Potassium (\(K\)) is more reactive. In group 1 (alkali metals), \(K\) is more reactive than \(Na\) (down the group reactivity increases), and compared to \(Mg\) (group 2) and \(Ca\) (group 2, \(K\) is more electropositive as alkali metals are more electropositive than alkaline earth metals in general).
• H: Sodium (\(Na\)) is more reactive. Among \(Be\) (group 2), \(Li\) (group 1), \(Na\) (group 1), \(Mg\) (group 2), in group 1, \(Na\) is more reactive than \(Li\) (down the group reactivity increases), and group 1 elements (alkali metals) are more reactive than group 2 (alkaline earth metals) in general.

Answer:

A. 1. Nitrogen, 2. Tellurium, 3. Aluminum, 4. Iodine
B. 1. Neon, 2. Krypton, 3. Arsenic, 4. Aluminum
C. 1. Chlorine, 2. Strontium, 3. Potassium, 4. Fluorine
D. 1. Barium, 2. Chlorine, 3. Oxygen, 4. Cesium
E. Circle: \(Cl\), Box: \(Se\)
F. \(N\)
G. \(K\)
H. \(Na\)