A nonpolar covalent bond, because the atoms are the same element.
The forces which hold a metal together are called metallic bonds. They consist of delocalised electrons which bind all the atoms together.
The liquid particles, if molecules, have bonds which hold the ATOMS together in the molecule. There are also intermolecular forces of attraction BETWEEN the molecules.
Metals are held together by metallic bonds. Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions. These bonds are the forces of attraction that hold metals together. Metals are made up of closely packed cations rather than neutral atoms. The valence electrons of metal atoms can be modeled as a sea of electrons. The valence electrons are mobile and can drift freely from one part of the metal to another. Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions. These bonds are the forces of attraction that hold metals together.
The factor that has the greatest effect on the melting point of a crystalline solid is the type of bonding among the particles. Heat breaks the bonds that hold the particles together.
To hold the fabric together while they sew.
covalent bonds
Covalent bonds hold atoms together. Ionic bonds hold ions together
Covalent bonds, specifically two double bonds, two sigma two pi bonds.
Bonds hold atoms together. There are hydrogen bonds, ionic bonds, and covalent bonds.
The three types of chemical bonds that hold the atoms within a compound together are Ionic bonds, Covalent bonds, and Polar covalent bonds.
The three types of chemical bonds that hold the atoms within a compound together are Ionic bonds, Covalent bonds, and Polar covalent bonds.
Peptide bonds
bonds
Covalent bonds, in which atoms share valence electrons, and ionic bonds, in which electrons are transferred from one atom to another, are the types of bonds that hold atoms together.
hydrogen bonds, disulphide bonds
Hydrogen Bonds
Organic compounds have covalent bonds.