Chemistry Chapter: Chemical Bonds

The number of valence electrons in an atom determines how it will bond with other atoms, which affects its reactivity.

Electrons in the outermost energy level of an atom.

The attractive force holding atoms together.

Attraction between oppositely charged ions (positive and negative).

Attraction between oppositely charged ions.

Atoms share electrons to form a bond.

Compound formed from positive and negative ions.

Valence electrons in metals are mobile, forming a 'sea of electrons' holding the metal atoms together.

Atoms sharing valence electrons.

Represent chemical reactions, showing reactants and products.

An atom that has gained or lost electrons, giving it a positive or negative electric charge.

Atoms gain or lose electrons to achieve a full outermost electron shell, a stable configuration similar to noble gases.

Cations (positive ions) and anions (negative ions).

Metals lose electrons to form positively charged ions (cations).

Nonmetals gain electrons to form negatively charged ions (anions).

A shorthand representation of a molecule, showing the types and number of atoms present.

A one or two letter abbreviation representing an element, with the first letter capitalized and the second lowercase.

A number placed before a chemical formula, indicating the number of molecules present.

A number placed after an element symbol, indicating the number of atoms of that element in a molecule.

Used to enclose groups of atoms, indicating they are repeating as a unit.

A compound formed from only two elements.

LiBr

Magnesium (Mg) has a +2 charge, sulfur (S) has a -2 charge.

Ionic compounds have a strong, rigid structure due to the electrostatic attraction between oppositely charged ions. This structure makes them hard and brittle. When pressure is applied, the layers of ions can slide past each other, breaking the bonds.

When ionic compounds melt or dissolve, the ions become free to move, allowing them to carry an electric current. In their solid state, ions are fixed in a lattice and cannot move freely.

Covalent bonds involve the sharing of electrons between atoms. This sharing creates a strong attraction between the atoms, holding them together. Covalent compounds can exist as solids, liquids, or gases.

Metals have a unique bonding structure called metallic bonding. In this structure, valence electrons are free to move throughout the metal, creating a 'sea of electrons'. These free electrons can carry an electric current.

Metallic bonds involve the sharing of valence electrons between all the atoms in a metallic structure. This creates a strong attraction that holds the atoms together in a close-packed arrangement.

A group of atoms covalently bonded together that carries an overall positive or negative charge.

A compound containing both ionic and covalent bonds; the polyatomic ion acts as a single unit with an overall charge.

Distinguishing between ionic, covalent, or both types of bonds based on the elements involved in the compound.

A diagram showing only the valence (outermost) electrons of an atom.

Atoms tend to gain, lose, or share electrons to have 8 valence electrons (except hydrogen, which wants 2) like the nearest noble gas.

Shared pairs of electrons between atoms in a molecule.

Pairs of electrons in a Lewis Dot Structure that are not involved in a bond.

Carbon typically forms 4 covalent bonds.

It tells you the typical number of bonds formed by hydrogen, oxygen, nitrogen, and carbon.

Hydrogen only needs one more electron to fill its outermost shell, so it's similar to halogens, which also need one electron.

A shorthand notation that shows the types and number of atoms in a molecule.

Chlorine has 7 valence electrons. Draw its symbol (Cl) and place 7 dots around it, starting with one dot on each side and then pairing them up.

The molecular formula for ammonia is NH3. This means it contains one nitrogen atom and three hydrogen atoms.