Atomic Structure/Periodic Table

Question 1

Atomic number

Answer 1

• The number of protons in an atom’s nuclei

Question 2

Mass Number

Answer 2

• The mass of one particular isotope
• The protons and neutrons of a isotope

Question 3

How do you find the neutron number of an isotope when you have the Atomic number and mass number?

Answer 3

Mass number - Atomic number = Neutrons

Question 4

Isotope

Answer 4

• Atoms of the same element with different numbers of neutrons
• Same Atomic number, different atomic mass

Question 5

Ion

Answer 5

• Atoms that have gained or lost electrons
• Ruins balance of protons and electrons, thus having a negative or positive charge

Question 6

Electronegativity

Answer 6

• Scale to represent how much the atom wants electrons

Question 7

Ionic Bond

Answer 7

• A metal atom gives an electron to a non-metal electron to have a stable/full shell
• EN is greater than 1.7

Question 8

Covalent Bond

Answer 8

• Two non-metal atoms share electrons to have a stable/full shell
• EN is less than 0.4

Question 9

Polar Covalent Bond

Answer 9

• Two non-metal atoms with different ENs share electrons unevenly to have a stable/full shell
• An extreme Polar covalent bond is an ionic bond
• EN is greater than 0.4 but less that 1.7

Question 10

Bonding Pair

Answer 10

• The pairs of electrons shared in Covalent bonding

Question 11

Lone Pair

Answer 11

• The pairs of electrons not involved in the sharing process of Covalent bonding

Question 12

Atomic mass

Answer 12

• Units used to represent the mass (weight without gravity) of elements
• Based off of Hydrogen 1
• Average number of protons and neutrons for isotopes of the element
• Approximate to Mass number
• Early Periodic Tables were ordered by increasing Atomic mass

Question 13

Periods

Answer 13

• Horizontal
• Number of electron shells
  Ex. Row 3 = 3 electron shells
• Periods span across long ——– spans of time

Question 14

Order of Families

Answer 14

Alkali metals(Needs to give away one electron to be stable, 2nd most reactive), Alkali earth metals, transition metals, representative metals, Metalloid(Elements surrounding this staircase have metal and non-metal properties), Halogens(Need one electron to be stable, very reactive), Noble gases(Full valence shells, very low reactivity)

Question 15

What are the two lower rows called?

Answer 15

Lanthanides and Actinides

Question 16

How do you read electron shells from the periodic table?

Answer 16

• Rows goes from 2 - 8- 18 - 32
• 3rd and 4th row have a hole shape
• 3rd role includes Lanthanides

Question 17

Families

Answer 17

• Elements in the same columns have similar properties
• The similarities are more obvious the more you move down the table
• Up Down (That one tall family)

Question 18

Trends in Atomic Radii (How big the atom is)

Answer 18

• Excluding Noble gases, size increases as you go left/bottom

Question 19

Trends in Ionization Energy (Energy needed to give away Electrons)

Answer 19

• The fuller the valence shell (To the right), the higher the Ionization energy
• The smaller the atomic mass is, the higher the ionization energy

Question 20

Metallic character

Answer 20

• Like the Atomic Radii, they increase as you go left/bottom