PERIODIC TABLE Kenneth E. Schnobrich

Li Atomic Mass Oxidation State Atomic Number Electron Configuration 3 6.941 +1 Atomic Number 3 1s22s1 or 2-1 Electron Configuration

GROUPS H Li Na K Rb VERTICAL COLUMNS - • Alkali Metals • Alkaline Earth Metals • Transition Elements • Chalcogens • Halogens • Inert (Noble) Gases 1 2 3-12 16 17 18 Li Na K Rb

PERIODS 1s22s1 1s22s2 1s22s22p1 1s22s22p2 1s22s22p3 HORIZONTAL ROWS - the Period Number indicates the Principal Energy Level that is filling as we move from left to right. Li Be B C N O F Ne

PERIODS 2-1 2-2 2-3 2-4 2-5 2-6 2-7 2-8 HORIZONTAL ROWS - the Period Number indicates the Principal Energy Level that is filling as we move from left to right. Li Be B C N O F Ne

METALS METALLOIDS NONMETALS INERT GASES

Atomic Radius Table S* DECREASES *NYS Reference Tables for Chemistry

COVALENT RADII - PERIOD 2

Atomic Radius INCREASES

COVALENT RADII - GROUP IA

Types of Atomic Radii Covalent Radius - effective distance from the center of the nucleus to the outer valence shell in a covalent or coordinate covalent bond. Van der Waals Radius - half the closest distance between two nonbonded atoms.

Metals + Loss of electrons - Nonmetals Gain of electrons

IONIZATION ENERGY ELECTRONEGATIVITY Definitions Ionization Energy – the amount of energy (usually in kilojoules) needed to remove the most loosely bound electron from a gaseous atom of an element. Electronegativity – the attractive force that an atom has for an electron(s) during the formation of a chemical bond. (no units are assigned)

Ionization Energy & Electronegativity “PROPERTIES OF SELECTED ELEMENTS” Table S First Ionization Energy (kJ/mol) Na 496 0.9 Electronegativity

Ionization Energy INCREASES

General Trend Across a Period

Ionization Energy DECREASES

General Trend Down a Group

General Trend Down a Group

ELECTRONEGATIVITY DECREASES Table S* *NYS Reference Tables for Chemistry

Electronegativities of Group IA

Electronegativity Across a Period INCREASES

Electronegativities for Period 2

REACTIVITY REACTIVITY INCREASES REACTIVITY INCREASES

Transition Elements Multiple Oxidation States Form Colored Compounds Incomplete Inner “d” Sublevels

TYPICAL QUESTIONS

The Most active metals are in Group - 1 (IA) 15 (VA) 13 (IIIA) 17 (VIIA)

The elements known as Alkali metals are found in Group 1 (IA) 2 (IIA) 13 (IIIA) 17 (VIIA)

What is the total number of electrons found in the valence shell of an Alkaline Earth element in the ground state 1 2 3 4

As the elements in Group IIA are considered from top to bottom, the # of electrons in the 2s subshell increases decreases remains the same

Which group contains atoms that form +1 ions having an inert gas configuration? 1 (IA) 11 (IB) 17 (VIIA) 7 (VIIB)

Which Group 17(VIIA) elements listed below has the greatest nuclear charge? F Cl Br I

Which element is most likely to form a compound with Kr? Fluorine Chlorine Bromine Iodine

Which group on the Periodic Table contains solid, liquid, and gaseous elements at room temperature? 2 (IIA) 16 (VIA) 17 (VIIA)

Which represents the correct order of activity for the Group VIIA(17) elements? Br > I > F > Cl F > Cl > Br > I I > Br > Cl > F F > Br > Cl > I

If the elements are considered from top to bottom in Group 16(VIA), the number of electrons in the outermost shell will? decrease increase remain the same

Which Group contains and element that is a liquid at room temperature? 2 (IIA) 11 (IB) 12 (IIB)

Which element has the greatest tendency to gain electrons? Se S O USE CHART S

When atoms of the elements in Group 18 (0) are compared in order from top to bottom, the attractions between atoms? increases and the boiling point decreases decreases and the boiling point increases increases and the boiling point increases decreases and the boiling point decreases

In the ground state, an atom of which element in Period 3 has the most loosely bound electron? Si Na S Ar USE CHART S

Which Period contains elements that are all gases at STP? 1 2 3 4

Considered in succession, the elements in Period 2 of the Periodic Table show a decrease in atomic radius with increasing atomic charge increases? nuclear charge increases # of PEL increases number of neutrons decreases # of protons increases

Which represents the electron configuration of a metalloid in the ground state? 2-3 2-5 2-8-5 2-8-6

In a given Period of the Periodic Table, the element with the lowest first ionization energy is always? an Alkaline Earth Metal an Alkali Metal a Halogen an Inert Gas USE CHART S

As one goes from Li to F in Period 2 of the Periodic Table, the atomic radius of the elements? decreases increases remains the same USE CHART S

An element in which electrons from more than one energy level may be involved in bond formation? potassium calcium copper zinc

Which element can form more than one binary compound with chlorine? potassium calcium iron zinc

A pure compound is blue in color. It is most likely a compound of? sodium lithium calcium copper

Which is the electron configuration of a transition element in the ground state? 2-8-8 2-8-8-2 2-8-18-2 2-8-18-8 Ar Ca Zn Kr