Atomic and Electronic Structure

Question 1

group 1

Answer 1

excluding hydrogen, alkaline metals

Question 2

group 2

Answer 2

alkaline earth metals

Question 3

group 3-12

Answer 3

transition metals

Question 4

group 13-17

Answer 4

metalloids; combo of metallic and nonmetallic characteristics

Question 5

group 17

Answer 5

halogens

Question 6

group 18

Answer 6

noble gases

Question 7

metallic character trend

Answer 7

• increases from left to right
• increases going down

Question 8

atomic radius

Answer 8

1/2 distance between nuclei of 2 identical atoms bonded together

Question 9

atomic radius trend

Answer 9

• increases from right to left
• increases going down a group

Question 10

isoelectronic series

Answer 10

atoms that have the same electronic configuration but differing number of protons
* most positive charged atom will have the smallest radius because the most protons with the same number of electrons

Question 11

electron affinity

Answer 11

amount of energy released when an electron is added to an atom

Question 12

electron affinity trend

Answer 12

• increases from left to right
• decreases going down a group

Question 13

electronegativity

Answer 13

ability of an atom to attract an electron in a bond
* the greater the ability to attract an electron the greater the electronegativity

Question 14

electronegativity trend

Answer 14

• increases from left to right
• decreases going down a group

Question 15

electronegativity of noble gases

Answer 15

an exception because their valence shell is full therefore have NO electronegative value

Question 16

most electronegative atom

Answer 16

F

Question 17

diatomic elements

Answer 17

have no fear of ice cold bear
* hydrogen
* nitrogen
* fluorine
* oxygen
* iodide
* carbon
* boron??

Question 18

effective nuclear charge

Answer 18

nuclear charge experienced by an electron in an atom with multiple electron

Question 19

Zeff =

Answer 19

Z - S
* Z: number of protons
* S: number of shielding electrons

Question 20

effective nuclear charge trend

Answer 20

• increases from left to right
• decreases going down a group

Question 21

ionization energy

Answer 21

energy needed to remove and electron from an atom

Question 22

ionization energy trend

Answer 22

• increases from left to right
• decreases going down a group

Question 23

exception to ionization energy

Answer 23

• alkaline earth metals > group 13 because they have completely filled orbitals therefore requires more energy to remove electron
• group 15 > group 16 because group 15 has 1/2 filled orbitals which is a more stable configuration therefore also requires more energy to remove electron