Honors Chemistry Periodic Table Quiz

Dimitri Mendeleev

• Had elements arranged in order of increasing atom mass show similar chemical and physical properties

• This occurs at periodic intervals

• Modern Periodic Law: the physical and chemical properties of elements are periodic functions of their atomic numbers

Periods

Horizontal rows, the number of the period indicates the highest principal energy level with electrons(shells)

Groups(families)

vertical columns on periodic table

sum number of valence electrons means

similar properties

metals general definition

elements located to the left of the staircase(75% of the table)

metalloid general definition

elements adjacent to the staircase(excluding Al)

nonmetals general definition

elements located to the right of the staircase

common properties of metals

• solids at room temperature(excluding Hg)

• malleable

• ductile

• have luster

• good conductors of heat and electricity because of highly mobile valence electrons

• low ionization energy

• low electronegativity values

• need to lose electrons to form positive ions(cations) with smaller radii

Why do metals conduct electricity?

valence electrons in metals move freely throughout the structure

properties of nonmetals

• many are gases at room temperature(bromine is a liquid)

• some are network solid like diamond

• brittle

• solids are dull

• poor conductors of heat and electricity

• high ionization energy

• high electronegativity values

• tend to gain electrons to form negative ions(anions) with larger radii

Metalloids

• intermediate elements that display both metallic and nonmetallic properties

  • conduct electricity, but not as well as metals

  • shiny like metals but brittle like nonmetals

Noble Gases

• group 18

• unreactive

• have completely filled valence electrons shells

• stable electron configuration

• H & He = duet rule

Octet Rule

atoms will gain, lose, or share electrons in order to obtain a stable octet of electrons

Hydrogen

• doesn’t have properties similar to group 1(detached)

• nonmetal

• only element that can gain, lose, or share its one valence electrons to become stable

• can form a +1 or -1 ion

Group 1(alkali metals) and Group 2(alkaline earth metals)

• most reactive metals(group 1 > group 2, bottom of group > top of group)

• reactive metal means they easily lose their electrons

• can only be found in compounds in nature(free elements are produced by the electrolysis of the fused compounds)

Group 3-12: transition elements/metals

• outermost d sublevels are being filled(non valence electrons)

• typically hard solids with high melting points(except Hg)

• transition elements typically have multiple oxidation(ionic) states(e- lost from more than one energy level)

• less reactive than group 1 and group 2(copper, silver, gold are the least reactive)

• transition elements typically form colored ions in solution

Group 14(carbon group)

• structure = function

• nonmetals that typically form network solids

• carbon can have multiple forms in the same form(diamond vs. graphite)

allotropes

nonmetals that exist in two or more forms in the same phase. they have different chemical and physical properties because they have different structures(oxygen vs ozone and white vs red phosphorus)

Group 15 and Group 16

• nitrogen and oxygen are both diatomic

• BrINCl HOF

• nitrogen contains a triple bond

• oxygen contains a double bond

Group 17(halogens)

• in a compound they are called halides

• only group that contains all these phases of matter at room temperature

• most reactive of the nonmetals

• nonmetals react by gaining electrons

• the top of the group is more reactive than the bottom of the group

• can only be found in a combined state in nature(like group 1 and group 2)

Ion Formation for Groups

Group 1 - lose one electron, form a +1 ion

Group 2 - lose two electrons, form a +2 ion

Group 13 - lose three electrons, form a +3 ion

Group 16 - gain two electrons, form a -2 ion

Group 17 - gain one electron, form a -1 ion

number of e-s lost = number of e-s gained

atomic radius trend across a period

decreases

electronegativity trend across a period

increases

first ionization energy trend across a period

increases

metallic character(reactivity) trend across a period

decreases

nonmetallic character(reactivity) trend across a period

increases

atomic radius trend down a group

increases

electronegativity trend down a group

decreases

first ionization energy trend down a group

decreases

metallic character(reactivity) trend down a group

increases

nonmetallic character(reactivity) trend down a group

decreases

Why are periodic trends doing what they do down a group

more electron shells

Why are periodic trends doing what they do across a period?

more proton pull

how to find radius size

first, find what is positive and negative and sort accordingly

then, find the number of electrons