1. Chapter 5.2 – Exploring the Periodic Table
periodic trends on the periodic table are due to electron arrangement
the number of valence electrons determines chemical properties
an elements location is related to its electron arrangement s p
sublevel being filled d f

2. Chapter 5.2 – Exploring the Periodic Table
Group 1 and 2 fill the s sublevel
Group 1 has 1 valence electron
Group 2 has 2 valence electrons
Groups 13 – 18 fill the p sublevel, the s sublevel is filled
Group 13 has 3 valence electrons
Group 14 has 4 valence electrons
Group 15 has 5 valence electrons
Group 16 has 6 valence electrons
Group 17 has 7 valence electrons
Group 18 has 8 valence electrons

3. Chapter 5.2 – Exploring the Periodic Table
ion –
atom or molecule that has gained or lost one or more electrons and has a negative or positive charge
ions do not have equal numbers of protons and electrons
atoms want to fill their s and p sublevels and have 8 valence electrons
atoms gain 8 valence electrons by gaining or losing electrons
cation – positive ion
anion – negative ion

4. Chapter 5.2 – Exploring the Periodic Table
if an atom has 1, 2, or 3 valence electrons, the atom will lose electrons and form a positive ion
if an atom has 5, 6, or 7 valence electrons, the atom will gain electrons and form a negative ion
Lithium (Li) –
Group 1 – has 1 valence electron –
forms Li+ ion
Oxygen (O) –
Group 16 – 6 valence electrons –
forms O2- ion

5. Chapter 5.2 – Exploring the Periodic Table
metal – element that is shiny and conducts heat and electricity well - found on the left side of the periodic table - most elements are metals nonmetal – element that conducts heat and electricity poorly - found on the right side of the periodic table - most are gases

6. Chapter 5.2 – Exploring the Periodic Table
semiconductor or metalloid – element that conducts electric current better than an insulator but not as well as a conductor - shares properties with metals and nonmetals - found between metals and nonmetals on the periodic table