Question

question 33 1 pts which ion with a +2 charge has the electron configuration shown below: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ □ mg²⁺ □ ca²⁺ □ sr²⁺ □ be²⁺ question 34 1 pts which ion with a 3 - charge has the electron configuration shown below: 1s² 2s² 2p⁶ 3s² 3p⁶ □ p³⁻ □ n³⁻ □ as³⁻ □ al³⁻

Explanation:

Step1: Determine electron number for +2 ion

For an ion with a +2 charge, the neutral - atom has 2 more electrons. The given electron - configuration $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}$ has a total of $2 + 2+6 + 2+6 + 2+10 + 6=36$ electrons. The neutral - atom has $36 + 2=38$ electrons. The atomic number (number of protons) of the neutral - atom is 38, which is strontium (Sr). So the ion is $Sr^{2 + }$.

Step2: Determine electron number for 3 - ion

For an ion with a 3 - charge, the neutral - atom has 3 fewer electrons. The given electron - configuration $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$ has a total of $2 + 2+6 + 2+6=18$ electrons. The neutral - atom has $18-3 = 15$ electrons. The atomic number (number of protons) of the neutral - atom is 15, which is phosphorus (P). So the ion is $P^{3 - }$.

Answer:

Question 33: Sr²⁺
Question 34: P³⁻