C2.2 Bonding

Metals | non metals Shiny | dull High melt and boil point | low melt and boil point Malleable | brittle Ductile | not ductile Heat and electricity good conductors | heat and electricity bad conductors

Old group numbers from 1 to 0 IUPAC group numbers from 1 to 18

Table which all the elements are arranged in rows and columns. In order of increasing atomic number (modern periodic table). Metals on left Non metals on right.

Metals lose electrons to form + ions Non metals gain electrons to form - ions Metals DON’T react with each other Non metals react with each other to produce compounds that consist of molecules. Both may react with oxygen producing oxides Metal oxides dissolved in water make alkaline solution and non metal oxides produce acidic solutions.

Periods - horizontal - rows - Where each atom has the same number of occupied electron shells Groups - Vertical - columns - elements have similar properties due to the arrangement of their electrons. How many electrons per outer shell

Shows how the electrons are arranged in its atoms.

Outermost occupied electron shell.

Around the nucleus in shells - different shells can hold different numbers of electrons Shell - maximum number of electrons First - 2 Second - 8 Third - 8 Fourth - 18

Counting from hydrogen, period by period until you reach the element you want. Period 1: 2 electrons in outer shell Period 2: 8 electrons in outer shell Period 3: 6 electrons in outer shell

Electrically charged particle formed when an atom, group of atoms loses or gains electrons. Atom with equal numbers of protons and neutrons but has different number of electrons. The overall charge can be positive or negative (charged particles) Metals form + ions as they lose electrons Non metals gain electrons and form - ions.

Ions go inside brackets Element symbol written in the centre Dots in element 1 crosses in element 2 to represent the electrons

Electrons are transferred from the metal’s atoms to the non metal’s atoms.

Contain positive and negative ions arranged in a regular way. This arrangement is giant ionic lattice Giant = arrangement repeated many times Ionic = Held in place with ionic bonds, that act in all directions Are strong electrostatic forced of attraction Lattice = arrangement is regular and not random. Happens between a metal and non metal formed when one or more outer shell electrons are transferred from metal atom to non - metal atom

Shared pair of electrons to complete each atom’s outer shell Happens between 2 non metals involve electrostatic forces of attraction between the nucleus of each bonded atom and the shared electrons Strong bonds

Particle in which non metal atoms are joined to each other with covalent bonds

Limitations: sizes of atoms and ions are inaccurate Shows that atoms or ions held by forces and not physical bonds atoms or ions too far apart Ion charges not shown

Each atom is represented by its chemical symbol Each covalent bond is a straight line Limitations: Does not show the 3D shape of the molecule.

Consists of many non-metal atoms joined by covalent bonds and arranged in a repeating regular pattern Have many atoms

Monomers Join end to end in chemical reactions

Simple molecules Few non metal atoms joined by covalent bonds

Chains Joined together by strong covalent bonds - cross linking

The polymer chains in the tangled web are easy to separate when energy is given to them.

Solid state at room temperature except from mercury Atoms packed together in a regular way forming a giant metallic lattice. Modelled by drawing circles or spheres arranged in a regular pattern, touching each other.

Metals lose electrons to form positive ions. Electrons leave the outer shells of the metal atoms, forming a “sea” of electrons around positively charged metal ions. These are free to move through the structure of the metal, so they are called delocalised electrons. The electrons from the outer shells of the metal atoms are delocalised, are free to move through the whole structure. This sharing of delocalised electrons results in strong metallic bonding. Strong electrostatic forces of attraction between the delocalised electrons and the closely packed positive metal ions.