Question

complete the following table. draw arrows between the lewis dot structures of the atoms to show where electrons are moving.
element | sodium | chlorine
group # (a#) | ia | viia

valence electrons | 1 | 7

easier to gain/lose e⁻ & how many | lose 1 | gain 1
lewis dot of atom | na· | :cl:
lewis dot of ion | na⁺ | :cl:⁻

e⁻ after gain/loss | 10 | 18

p⁺ after gain/loss | 11 | 17

atomic charge (oxidation number) | 1+ | 1-
cation or anion | cation | anion
ion name | sodium ion | chloride ion
ion symbol (include charge) | na⁺ | cl⁻
ionic compound formula | nacl |
ionic compound name | sodium chloride |

| potassium | fluorine
|----|----
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| selenium | calcium
|----|----
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Explanation:

Step1: Fill Potassium (Group IA)

Step1a: Group & valence electrons

Group IA, valence electrons = 1

Step1b: Electron behavior

Lose 1 electron

Step1c: Lewis Dot (Atom/Ion)

Atom: $\dot{K}$; Ion: $K^+$

Step1d: Electrons/protons post-change

$e^-$ after: 18; $p^+$ after: 19

Step1e: Ion properties

Charge: 1+; Cation; Ion Name: Potassium ion; Ion Symbol: $K^+$

Step1f: Ionic compound (with Cl)

Formula: $KCl$; Name: Potassium chloride

Step2: Fill Fluorine (Group VIIA)

Step2a: Group & valence electrons

Group VIIA, valence electrons = 7

Step2b: Electron behavior

Gain 1 electron

Step2c: Lewis Dot (Atom/Ion)

Atom: $\ddot{\underset{\cdot \cdot}{F}} \dot{}$; Ion: $\ddot{\underset{\cdot \cdot}{F}}:^-$

Step2d: Electrons/protons post-change

$e^-$ after: 10; $p^+$ after: 9

Step2e: Ion properties

Charge: 1-; Anion; Ion Name: Fluoride ion; Ion Symbol: $F^-$

Step2f: Ionic compound (with Na)

Formula: $NaF$; Name: Sodium fluoride

Step3: Fill Selenium (Group VIA)

Step3a: Group & valence electrons

Group VIA, valence electrons = 6

Step3b: Electron behavior

Gain 2 electrons

Step3c: Lewis Dot (Atom/Ion)

Atom: $\ddot{\underset{\cdot \cdot}{Se}} \dot{}\dot{}$; Ion: $\ddot{\underset{\cdot \cdot}{Se}}::^{2-}$

Step3d: Electrons/protons post-change

$e^-$ after: 36; $p^+$ after: 34

Step3e: Ion properties

Charge: 2-; Anion; Ion Name: Selenide ion; Ion Symbol: $Se^{2-}$

Step3f: Ionic compound (with Na)

Formula: $Na_2Se$; Name: Sodium selenide

Step4: Fill Calcium (Group IIA)

Step4a: Group & valence electrons

Group IIA, valence electrons = 2

Step4b: Electron behavior

Lose 2 electrons

Step4c: Lewis Dot (Atom/Ion)

Atom: $\dot{Ca}\dot{}$; Ion: $Ca^{2+}$

Step4d: Electrons/protons post-change

$e^-$ after: 18; $p^+$ after: 20

Step4e: Ion properties

Charge: 2+; Cation; Ion Name: Calcium ion; Ion Symbol: $Ca^{2+}$

Step4f: Ionic compound (with Cl)

Formula: $CaCl_2$; Name: Calcium chloride

Answer:

Category	Potassium	Fluorine	Selenium	Calcium
# Valence Electrons	1	7	6	2
Easier to gain/lose e⁻ & how many	lose 1	gain 1	gain 2	lose 2
Lewis Dot Of Atom	$\dot{K}$	$\ddot{\underset{\cdot \cdot}{F}} \dot{}$	$\ddot{\underset{\cdot \cdot}{Se}} \dot{}\dot{}$	$\dot{Ca}\dot{}$
Lewis Dot Of Ion	$K^+$	$\ddot{\underset{\cdot \cdot}{F}}:^-$	$\ddot{\underset{\cdot \cdot}{Se}}::^{2-}$	$Ca^{2+}$
# e⁻ after gain/loss	18	10	36	18
# p⁺ after gain/loss	19	9	34	20
atomic charge (oxidation number)	1+	1-	2-	2+
Cation or Anion	Cation	Anion	Anion	Cation
Ion Name	Potassium ion	Fluoride ion	Selenide ion	Calcium ion
Ion Symbol (include charge)	$K^+$	$F^-$	$Se^{2-}$	$Ca^{2+}$
Ionic Compound Formula	$KCl$	$NaF$	$Na_2Se$	$CaCl_2$
Ionic Compound Name	Potassium chloride	Sodium fluoride	Sodium selenide	Calcium chloride

Electron transfer arrows: For K & Cl: arrow from $\dot{K}$ to $\ddot{\underset{\cdot \cdot}{Cl}} \dot{}$; For Na & F: arrow from $\dot{Na}$ to $\ddot{\underset{\cdot \cdot}{F}} \dot{}$; For Na & Se: two arrows from two $\dot{Na}$ to $\ddot{\underset{\cdot \cdot}{Se}} \dot{}\dot{}$; For Ca & Cl: two arrows from $\dot{Ca}\dot{}$ to two $\ddot{\underset{\cdot \cdot}{Cl}} \dot{}$