Ch. 8 Periodic Trends

Question 1

What is periodic property?

Answer 1

• A property of an element based on its position on the periodic table

Question 2

What is the electron configuration?

Answer 2

-Quantum numbers described in shorthand

Question 3

What is Pauli Exclusion principle?

Answer 3

-No two electrons can have the same set of quantum numbers in a given atom

Question 4

What is the ascending size of the orbitals?

Answer 4

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Question 5

What is Coulombs Law?

Answer 5

• Interaction between charged particles

i. e. opposites attract and same charges repel

Question 6

What is the thought process to get out of Coulombs Law?

Answer 6

• As charged particles go apart r becomes increases but energy decreases
• As charges get closer r decreases and energy increases.

Question 7

What is Shielding?

Answer 7

-Repulsion of one electron that screen an outer orbital from the full effects of the nuclear charge

Question 8

What is the effective nuclear charge?

Answer 8

-The charge experienced by the outer orbital electrons from the nuclear charge with the shielding of inner electrons

Question 9

How do you calculate the effective nuclear charge?

Answer 9

Z(eff.) = Z ( charge of nucleus) - (Shielding of electrons)

Question 10

What is the degenerate?

Answer 10

-All the same energy levels with different orientation

Question 11

What is Aufbau principle in periodic trend?

Answer 11

-Start from the lowest energy orbital

Question 12

What is Hands rule with periodic trends?

Answer 12

-When there’s a degenerate orbitals place electron in each before pair 2 electrons

Question 13

What are the periodic trends for Effective nuclear charge?

Answer 13

• All groups (columns) have the same effective nuclear charge
• Left to right on a periodic table the effective nuclear charge increases

Question 14

What is the atomic radius?

Answer 14

-The distance form the electron from the nucleus

Question 15

What occurs to the atomic radius as the principal quantum numbers (n) increase?

Answer 15

-The electrons get further away form the nucleus

Question 16

What are the periodic trends with atomic radius?

Answer 16

• The atomic radius increases going down periodic tables columns
• Going to the right if n doesn’t change increasing effective nuclear charge decreases atomic radius, since electrons have a greater pull cause for a smaller radius

Question 17

What is ionization energy?

Answer 17

• The energy required to remove the highest energy electrons from a atom
• Is how easy to make a cation or pull off a valence electron

Question 18

What are the trend of ionization energy?

Answer 18

• Moving across the P.T. left to right increases I.E.

- Moving down a group decreases ionization energy

Question 19

Why does moving down a group result in a smaller ionization energy?

Answer 19

• Larger radius going down a column becomes easier to remove the outermost electrons
• Shielding- inner electrons block the attraction force of nucleus becomes more easy to remove an outer electron

-ex) holding a chair with body position away becomes easier for the chair to be removed

Question 20

What is electronegativity?

Answer 20

-Is how easy it is o give an atom a (-) charge i.e. make antion

Question 21

What is high electronegativity?

Answer 21

-An atom want an electron

Question 22

What are the trend on the periodic table with electronegativity?

Answer 22

-Move left to right on P.T. increases in E.N.

Question 23

What is the rule for transition metals electron configuration?

Answer 23

-The 4s is before the 3d

Question 24

What is paramagnetic?

Answer 24

-Unpaired electron and attracted to electric field

Question 25

What is diamagnetic?

Answer 25

-No unpaired electrons and not attracted to a magnetic field

Question 26

How should the equation for group 1 (alki metal) and group 7 (halogens) be written?

Answer 26

2Metal + Halogen( subscript 2) —> 2(Metal)(Halogen)

Question 27

How should the equation for group 2 (alki earth metal) and group 7 (halogens) be written?

Answer 27

Metal + (Halogen-subscript 2) –> (Metal)(Halogen-subscript 2)

Question 28

Why as you move across a P.T. the I.E. increases?

Answer 28

• The atomic radius decreases the outer most electrons are closer to the nucleus
• The effective nuclear charge increases which means there more of an attraction from the outer electron to the nucleus

Question 29

What is Lattice Energy?

Answer 29

-Energy associated with forming a crystalline lattice from gaseous state

Question 30

What is electron affinity?

Answer 30

• An atom or ion is the energy change associated with the gaining or an electron by the atom in the gaseous state.
• Atom usually releases energy