Bonding test

Electron Sea

Electron Sea

Metallic bonding happens between metal atoms when the atoms donate their valence electrons to a “pool” of shared valence electrons which can then flow around the atoms (now cations because they’re lost their valence electrons) and be shared by all of the atoms in the sample

Metallic bonds are the attractive forces between what?

Positive metal ions and moving valence electrons in a metal.

Metals are ____ at room temperature

Solids

Metallic bonds must have _____ forces of attraction between atoms.

Strong

Mixtures of metals are called?

Alloys

Metallic bonding happens between a group of…

Atoms and electrons that are shared by many atoms instead of being restricted to two atoms

Metals are malleable because…

of the free moving sea of electrons can easily adapt to new shapes

Metals are good conductors of electricity because…

the electrons in the sea are not fixed into a position but are free to carry a current

Metals are shiny because…

the sea of electrons provide a uniform surface that can absorb and reflect light uniformly

Types of atoms involved in ionic bonds

Metals and nonmetals

Types of atoms involved in covalent bonds

Nonmetals

Types of atoms involved in metallic bonds

Metals

Method of bond formation in ionic bonds

Transfer of electrons

Method of bond formation in covalent bonds

Sharing of electrons

Method of bond formation in metallic bonds

Sharing of transferred electrons

Type of structure in ionic bonds

Crystalline

Type of structure in covalent bonds

Molecular

Type of structure in metallic bonds

Crystalline

Physical state in ionic bonds

All solids

Physical state in covalent bonds

Mixture of solids, liquids and gases

Physical state of metallic bonds

All solids but mercury

Melting point of ionic bonds

Very high

Melting point of covalent bonds

Lower

Melting point of metallic bonds

High

Solubility in water for ionic bonds

Many are water soluble

Solubility in water for covalent bonds

Polar are water soluble, nonpolar are not

Solubility in water for metallic bonds

Not soluble in water

Electrical conductivity for ionic bonds

Good conductors when dissolved or melted

Electrical conductivity for covalent bonds

Non conductors

Electrical conductivity for metallic bonds

Very good conductors

Other properties of ionic bonds

Brittle

Other properties of covalent bonds

Includes organic compounds (a very large group of compounds)

Other properties of metallic bonds

Malleable, shiny

Dipole-Dipole occur between…

Polar molecules

London forces occur between…

All molecules but most important for non polar molecules

Hydrogen bonds occur between…

Every polar molecules in which hydrogen is bonded to Oxygen, Nitrogen or Fluorine

Dipole-Dipole relative strength

Intermediate

London forces relative strength

Weakest

Hydrogen bonds relative strength

Strongest

Brief explanation of Dipole-Dipole interaction

The positive regain on one polar molecule attract the negative region in another polar molecule

Brief explanation of London forces interaction

The constant shifting of electrons in the electron clouds of molecules produce temporary dipoles which can then briefly attract the temporary dipoles in other molecules. These forces increase with the size and number of electrons in a molecule

Brief explanation of Hydrogen bonds interaction

Similar to Dipole-Dipole forces but are much stronger because of the VERY polar molecules involved

Dipole-Dipole attractions are responsible for…

Higher melting and boiling points for polar compounds

London bonds are responsible for…

The ability of liquify a non polar substance like Oxygen or Nitrogen

Hydrogen bonds are responsible for…

The very high boiling point of water, the fact that ice floats, the ability of DNA to unzip and replace

Intermolecular forces

The forces that happen between molecules

Intramolecular forces

The forces that are within the bonds that hold molecules together

Chemical bond

An electrostatic force of attraction between two atoms that holds the atoms together.