Periodic TrendsPeriodic (adjective) Having a repeating pattern; happening again and again.
Examples: Day Night Day Periodic waves washing onto a beach at regular intervals.
Use patterns to predict future events or missing information like undiscovered elements. (You do not need to write this)How is the current periodic table organized? By Atomic Number (left to right)# protonsBy Column (group or family)- elements in the same column have the same number of valence electronsValence electrons-the electrons in the outer most electron shell.By row (period)- elements in the same period have the same number of electron shellsFamilies of Elementsare arranged by vertical column
Families are also called groupsDown A GroupAll elements in the same group (vertical column) on the periodic table have the same number of outer electrons (valence electrons)The number of valence electrons is dependent on which tall column in which the atom is located. 1st tall column =1 valence electron, 6th tall column = 6 valence electrons.Skip the shorter d block (10 shorter columns in the middle.
Elements in the same familyreact the same way.
This is because they pick upor give away the samenumber of electrons as othermembers of the family.Why do elements react?Elements react in a way to fill the outermost shell with 8 electrons.Noble gases are said to be perfect the way they are because they already have 8 valence electrons-this is why they rarely react with other elements.Give away or take electrons? In General
Fewer than four valence electrons - give away
More than four valence electrons - takeNaClNa+Cl-Give away electrons makes the element positive (called a cation)Take electrons makes the element negative (called an anion)Chemical FamiliesColumn 1 Li, Na, K Alkali MetalsColumn 2Be, Mg, Ca Alkaline Earth MetalsColumns 3-12Sc Zn Transition MetalsColumn 13B, Al, Ga Boron familyColumn 14C, Si, Ge Carbon familyColumn 15N, P, As Nitrogen familyColumn 16O, S, Se ChalkogensColumn 17F, Cl, Br HalogensColumn 18He, Ne, Ar Noble Gases
Across a periodAll elements in the same period (horizontal row) on the periodic table have the same number of electron shellsThe number of shells is dependent on the period in which the element is located. Peirod 1 = 1 shell, period 5 = five shells
There are many representations of the periodic table.some look more like what you are familiar with than others.
http://z.about.com/d/chemistry/1/0/0/W/mendeleevperiodic.jpgThe first periodic table
http://en.wikipedia.org/wiki/Image:Elementspiral.svgA spiral form of the periodic tableThis example was devised by Theodor Benfey and depicts the elements as a seamless series with the main group elements radiating from the center with the d- and f-elements filling around loops. 14
Metals, Non-metals and Metalloids
How could we test a sample to find out whether it is a metal, non-metal or metalloid?Most metals are not magneticWhat are some of the key properties of these groups?MetalsA metal is an element that is a good conductor of heat and electricity.At room temperature, most metals are solids.Most metals are malleable ( can be hammered or rolled into thin sheets).Metals tend to be ductile (can be stretched into fine wire).
SodiumCopperGoldNonmetalsA nonmetal is an element that is a poor conductor of heat and electricity. Many nonmetals are gases at room temperatureOne-bromine is a liquidThe solid nonmetals are brittle rather than malleable and ductile.
SulfurChlorineBromineMetalloidsA metalloid is an element that has some characteristics of metals and some characteristics of nonmetals.Metalloids are found along the stair-step line separates the metals from non-metals on the periodic table.They are semi-conductors of electricity.They are all solids and tend to be less malleable than metals but not as brittle as nonmetals
SiliconBoronWhen elements combine:Metal + non-metal ionic bond (lose and gain electrons-ionic compound-formula unit)
Non-metal and non-metal (share electrons-covalent bond-molecule)Other common Periodic TrendsAtomic Radius one-half the distance between the nuclei of identical atoms that are bonded together.Ionization Energy (IE)- The energy required to remove one electron from a neutral atom of an element.Electron affinity- The energy change that occurs when an electron is acquired by a neutral atom.Electronegativity- a measure of the ability of an atom in a chemical compound to attract electrons.