Gen Chemistry Ch 2: The Periodic Table

Question 1

Periodic Table of the Elements

Answer 1

Organize the elements according to their atomic numbers and reveals a pattern of similar chemical and physical properties among elements

Question 2

Periods

Answer 2

Rows within the periodic table, are based on the same principle energy level (n), seven of them (n=1 t0 n=7 for s and p block)

Question 3

Groups

Answer 3

Columns within the periodic table, elements in the same group have the same valence shell electron configuration, share similar chemical properties

Question 4

Three types of elements

Answer 4

Metals, nonmetals, and metalloids

Question 5

Metals

Answer 5

Shiny, conduct electricity well, are malleable and ductile, found on the left side in the middle of the periodic table, low effective nuclear charge, low electronegativity, high electropositivity, large atomic radius, small ionic radius, low ionization energy, and low electron affinity (can easily give up electrons)

Question 6

Nonmetals

Answer 6

Dull, poor conductors of electricity, and brittle, found on the right side of the periodic table, high ionization energy , high electron affinity, high electronegativity, small atomic radii, large ionic radii, unable to give up electrons easily, less unified in chemical and physical properties than metals

Question 7

Metalloids

Answer 7

aka semimetals, possess characteristics of both metals and nonmetals and are found in a stairstep pattern starting with boron, electronegativities and ionization energies in the middle and other physical properties vary, reacitivies depends on elements they are reacting with

Question 8

Effective nuclear charge

Answer 8

Zeff - net positive charge experienced by electrons in the valance shell in forms the foundation for all periodic trends, increased from left to right across a period with little change from top to bottom in a group, electrostatic attraction between the valence shell electrons and the nucleus

Question 9

Atomic radius trend

Answer 9

Equal to one-half the distance between the centers of two atoms of an element that are briefly in contact with each other, decreases from left to right across a period and increases from top to bottom in a group

Question 10

Ionic radius

Answer 10

Size of a charged species, largest nonmetallic ionic radii and the smallest metallic ionic radii exist at the metalloid boundary, cations generally smaller than their neutral atom, anions are generally larger than their neutral atom

Question 11

Ionization energy

Answer 11

The amount of energy necessary to remove an electron from the valance shell of a gaseous species, increases from left to right across a period and decreases from top to bottom in a group

Question 12

Electron affinity

Answer 12

The amount of energy released when a gaseous species gains an electron and in its valance shell, increases from left to right across a period and decreases from top to bottom in a group

Question 13

Electronegativity

Answer 13

A measure of the attractive force of the nucleus for electrons within a bond, increases from left to right across a period and decreases from top to bottom in a group, relative measurement, many scales

Question 14

Alkali metals

Answer 14

Typically take on an oxidation state of +1 and prefer to lose an electron to achieve a noble gas-like configuration, they in the alkaline earth metals are the most reactive of all metals, low Zeff, large atomic radii, low ionization energy, low electron affinity, low electronegativity, an active metal

Question 15

Alkaline earth metals

Answer 15

Take on an oxidation state of +2 and can lose two electrons to achieve a noble gas-like configurations, an active metal

Question 16

Chalcogens

Answer 16

Take on an oxidation state of -2 or +6 (depending on whether they are nonmetals or metals) in order to achieve noble gas configurations, very biologically important, generally small atomic radii and large ionic radii

Question 17

Halogens

Answer 17

Take on an oxidation state of -1 and prefer to gain an electron to achieve noble gas-like configurations, these nonmetals have the highest electronegativities, typically found as halides, physical properties vary

Question 18

Noble gases

Answer 18

aka inert gases, have a fully filled valance shell and their standard state and preferred not to give up or take on additional electrons, they are very high ionization energies and some have virtually nonexistent electronegativities and electron affinities, low boiling points, gas at room temperature

Question 19

Transition metals

Answer 19

Unique because they take on multiple oxidation states, which explains their ability to form colorful complexes with nonmetals of varying solubility and solution and their utility in certain biological systems, many have two or more oxidation states, some relatively nonreactive, low electron affinity, low ionization energy, low electronegativity, malleable, good conductors, high melting and boiling points

Question 20

Periodic law

Answer 20

Periodic table is a visual representation of it, states that the chemical and physical properties of the elements are dependent, in a periodic way, upon their atomic numbers

Question 21

A elements

Answer 21

aka representative elements, have valance electrons in the orbitals of either s or p subshells

Question 22

B elements

Answer 22

aka non representative elements, include transition elements (have valance electrons in s and d) and the lanthanide and actinide series (have valance electrons in s and f)

Question 23

Oxidation states

Answer 23

Charges when forming bonds with other atoms

Question 24

Malleability

Answer 24

Ability of a metal to be hammered into shaped

Question 25

Ductility

Answer 25

The ability of a metal to be pulled or drawn into wires

Question 26

Active metals

Answer 26

Groups 1 and 2, such low ionization energies that they do not exist naturally in their neutral forms

Question 27

First ionization energy

Answer 27

The energy necessary to remove the first electron, lower than the second ionization energy

Question 28

Halides

Answer 28

Ions of halogens, typical state of halogens