Complete and balance this equation for a combination reaction.

Be + O2 ==>

Would it be Be + O2 ==> BeO2 ?
or... 2Be + O2 ==> 2BeO ? Why??

The reaction is

Be + O2 ==> BeO. Be is in group II, O is in group VI (or 16 depending upon the system you are using); therefore, the formula is BeO. To balance,
2Be + O2 --> 2BeO

The balanced equation for the combination reaction of beryllium (Be) and oxygen (O2) can be determined by considering the valence electrons of each element.

Beryllium has a valency of 2, meaning it can form 2 bonds or gain 2 electrons to achieve stability. Oxygen, on the other hand, has a valency of 2 as well and can form 2 bonds or gain 2 electrons as well.

With this information, we can write the balanced equation as:

2Be + O2 ==> 2BeO

In this equation, two beryllium atoms react with one molecule of oxygen (O2) to form two molecules of beryllium oxide (BeO). By balancing the equation in this manner, we ensure that each side of the reaction has an equal number of atoms, therefore satisfying the law of conservation of mass.

To balance the given equation for a combination reaction, let's follow the steps:

Step 1: Write down the unbalanced equation:
Be + O2 ==> ?

Step 2: Determine the number of each type of atom on both sides of the equation.
On the left side, we have 1 atom of Be and 2 atoms of O.
On the right side, we don't know the number of atoms yet.

Step 3: Balance the equation by adjusting the coefficients.
To balance the equation, we need to make sure that the number of each type of atom is equal on both sides.

If we write it as Be + O2 ==> BeO2, the number of oxygen atoms would be 2 on the right side but only 1 on the left side. This equation is unbalanced.

Therefore, we need to balance the equation as 2Be + O2 ==> 2BeO. By doing this, we have 2 atoms of Be and 2 atoms of O on both sides.

So, the correct balanced equation for the combination reaction involving Be and O2 is:
2Be + O2 ==> 2BeO.