what determines the ability of atoms to bond together to form molecules?

Answer 1

the number of valence electrons.

Answer 2

In a polar compound an atom of a polar bond attracts more the bonding electrons than the other> This gives rise to an electrical dipolar moment> Ex : Molecule of HCl gaseous Cl is a very strong electronegative atom > In its bonding with the elctropositive atom H , The atom Cl has a negative electrostatic charge while the H is positive

Answer 3

The number and nature of their electrons.

Ionic bonds, for example, work by having two atoms, one lacking an electron and one having an excess electron, share an electron to form a bond.

There are a few different kinds of bonds, so there's room for a few answers here.

Answer 4

It's the number of unpaired electrons they have in their outer atomic orbitals. These are needed to form molecular bonds.

Two unpaired electrons (one in each atom) are bonded together to create a molecular orbital. Two electrons in a molecular orbital are more stable than two single electrons in two atomic orbitals so this encourages the formation of bonds between atoms. Nature is always seeking the most stable situation for electrons, the lowest energy state.

Answer 5

Their ability to give or share electrons with other atoms. The more tightly they hold their electrons the less likely they are to bond to other atoms. The more loosely they hold their electrons the more reactive they'll be.

Answer 6

Valence electrons and electron shells. Atoms want to get their completed shell set: 2, 8, 16, etc. So they either want to dump electrons (reduction agents) or take 'em (oxidation agents).

Answer 7

Octet rule: in general atoms want a full 8 valence cloud (unless it is hydrogen)

Answer 8

It all depends on positive ions, and negitive ions and how many electons and how many protons you are workin with

Answer 9

attraction/ repulsion forces