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 pd
f
sublevel being filled
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
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
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
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
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
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