BALANCING CHEMICAL EQUATIONS

1. ___ H2 + ___ O2 → ___ H2O
2. ___ Mg + ___ O2 → ___ MgO
3. ___ Li + ___ F2 → ___ LiF
4. ___ K + ___ O2 → ___ K2O
5. ___ H2O2 → ___ H2O + ___ O2
6. ___ Al + ___ Cl2 → ___ AlCl3
7. ___ Ag2O → ___ Ag + ___ O2
8. ___ H2 + ___ N2 → ___ NH3

1. _2_H2 + ___ O2 → _2_ H2O

2. _2_ Mg + ___ O2 → _2_ MgO

3. _2_ Li + ___ F2 → _2_ LiF

4. _4_ K + ___ O2 → _2_ K2O

5. _2_ H2O2 → _2_ H2O + ___ O2

6. _2_ Al + _3_ Cl2 → _2_ AlCl3

7. _2_ Ag2O → _4_ Ag + ___ O2

8. _3_ H2 + ___ N2 → _2_ NH3

Explanation:

1. 2 and 1=2

2. 2 and 1=2

3. 2 and 1=2

4. 4 and 1=2

5. 2=2 and 1

6. 2 and 3=2

7. 2=4 and 1

8. 3 and 1 =2

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.