Question

1. practice: use the gizmo to create stable compounds from the combinations given below. after transferring electrons, arrange the atoms to demonstrate the attraction between positively charged ions and negatively charged ions. click check to check each compound.

for each compound, click the camera ( ) icon to take a snapshot. right - click the image, and click copy image. paste each image into a blank document to turn in with this worksheet. write the ionic charges (such as ca²⁺) and chemical formulas below.

a. lithium and fluorine: li f
b. beryllium and oxygen: be o
c. magnesium and fluorine: mg f
d. aluminum and chlorine: al cl

Explanation:

Step1: Determine ionic charges based on electron - transfer

Lithium (Li) has 1 valence electron and loses it to achieve a stable configuration, forming $Li^+$. Fluorine (F) has 7 valence electrons and gains 1 electron to achieve a stable configuration, forming $F^-$. The chemical formula is LiF.

Step2: Analyze beryllium and oxygen

Beryllium (Be) has 2 valence electrons and loses them to form $Be^{2 + }$. Oxygen (O) has 6 valence electrons and gains 2 electrons to form $O^{2 - }$. The chemical formula is BeO.

Step3: Examine magnesium and fluorine

Magnesium (Mg) has 2 valence electrons and loses them to form $Mg^{2+}$. Fluorine (F) gains 1 electron to form $F^-$. Since Mg loses 2 electrons and each F gains 1 electron, the chemical formula is $MgF_2$.

Step4: Consider aluminum and chlorine

Aluminum (Al) has 3 valence electrons and loses them to form $Al^{3+}$. Chlorine (Cl) has 7 valence electrons and gains 1 electron to form $Cl^-$. Since Al loses 3 electrons and each Cl gains 1 electron, the chemical formula is $AlCl_3$.

Answer:

A. Ionic charges: $Li^+$, $F^-$; Chemical formula: LiF
B. Ionic charges: $Be^{2+}$, $O^{2 - }$; Chemical formula: BeO
C. Ionic charges: $Mg^{2+}$, $F^-$; Chemical formula: $MgF_2$
D. Ionic charges: $Al^{3+}$, $Cl^-$; Chemical formula: $AlCl_3$