Chapter 6

Question 0

What do the colors an element is written in stand for?

Answer 0

• Black: Solid at room temp
• Red: Gas at room temp
• Blue: Liquid at room temp
• Grey: Do not exist in nature

Question 1

What does the vertical column of numbers on a element on the periodic table stand for?

Answer 1

-The number of electrons in each occupied energy level

Question 2

Noble Gases

Answer 2

• The elements in Group 8A of the periodic table
• Also called inert gases because rarely take part in chemical reaction
• The s and p sublevels (if they have a p sublevel) are completely filled with electrons

Question 3

Representative Elements

Answer 3

• Group 1A to 7A on the periodic table
• Called this because have a wide range of physical and chemical properties
• Are either metals, metalloids or nonmetals
• Most are solids, some are gases, and only one (bromine) is a liquid at room temp.
• The s and p sublevels of the highest energy level are not filled

Question 4

Transition Elements

Answer 4

• All the Group B elements (entire D block)
• Two types: Transition metals and inner transition metals
• Used to be referred to as “rare earth metals”–> misleading because some transition metals are more abundant than other elements, and some inner transition metals cannot be found in nature

Question 5

Transition Metals

Answer 5

• Part of Group B on the periodic table
• Displayed in the main body of the periodic table
• The highest occupied s sublevel and a nearby d sublevel contain electrons
• Characterized y the presence of electrons in d orbitals

Question 6

Inner Transition Metals

Answer 6

• Below the main body of the periodic table
• The highest occupied s sublevel and a nearby f sublevel generally contains electrons
• Characterized by the presence of electrons in f orbitals

Question 7

Alkali metal

Answer 7

-Any metal in Group 1A of the periodic table

Question 8

Alkaline Earth Metal

Answer 8

• Any metal in Group 2A of the periodic table

Question 9

Halogen

Answer 9

-A nonmetal in Group 7 of the periodic table

Question 10

Periodic tables contain what?

Answer 10

• Each element’s name
• Symbol
• Atomic number
• Atomic mass
• Number of electrons in each energy level

Question 11

How can an elements electron configuration be determined?

Answer 11

-By its location on the periodic table

Question 12

Atomic Radius

Answer 12

• One-half of the distance between the nuclei of two atoms of the same element when the atoms are joined
• Measured in picometers

Question 13

Ion

Answer 13

• An atom or group of atoms that has a positive or negative charge
• Form when electrons are transferred between atoms
• Positive ion: Cation
• Negative Ion: Anion

Question 14

Cation Charge

Answer 14

• Positive
• Written as the number for the charge and a plus sign
• If the charge is 1, just used a plus sign

Question 15

Anion Charge

Answer 15

• Negative Charge
• Usually written as the number of the charge and a negative sign
• If the charge is 1, just a negative sign is used

Question 16

What type of elements tend to form anions, and what type of elements tend to form cations?

Answer 16

• Nonmetals form anions

- Metals form cations

Question 17

Ionization Energy

Answer 17

• The energy required to remove an electron from an atom

Question 18

First ionization Energy

Answer 18

-The energy required to remove the first electron from an atom

Question 19

Who made the periodic table

Answer 19

• Dimitri Mendeleev

- Ordered in increasing atomic mass

Question 20

Cations are always…

Answer 20

smaller than the atoms from which they form

-size decreases across period

Question 21

Anions are always…

Answer 21

larger than the atoms from which they form

-size decreases across period

Question 22

Ionic Size

Answer 22

-The size of an atom after receiving or removing an electron(s)

Question 23

Electronegativity

Answer 23

• The ability of an atom of an element to attract electrons when the atom is in a compound or molecule
• Lowest .7, highest 4.0

Question 24

Electron Shielding

Answer 24

• The one of the two forces that effect atomic size
• how electrons are attracted to the nucleus
• the more the valence electrons are blocked from the nucleus by other electrons
• This makes atoms larger^^
• Electron Shielding is dominant over Nuclear Charge
• constant across period, increases across group

Question 25

Metals

Answer 25

• 80% of periodic table
• Good conductors of heat and electricity (best= silver, second best= copper)
• Freshly cleaned metal will have a sheen (can reflect light)
• All metals are a solid @ room temp. (except mercury)
• Metals= ductile (can be turned into wire)
• Most metals= malleable ( able to be made into sheets without breaking)

Question 26

Nonmetals

Answer 26

• Most nonmetals are gases @ room temp
• few= solids (phosphorus, sulfur)
• Nonmetal that is liquid= bromine
• Because of many different types of nonmetals, no set characteristics
• Hard non-metals (diamond), brittle (break if hit)nonmetals (phosphorus)
• Poor conductors of heat & electricity

Question 27

Metalloids

Answer 27

• Has properties similar to metals and nonmetals
• Under some conditions, act like metals, in other conditions act like nonmetals
• Poor conductor of electricity

Question 28

Core electrons

Answer 28

• The electrons blocking the valence electrons

- Part of the inner energy levels

Question 29

Nuclear Charge

Answer 29

• One of the two forces that effect atomic size
• How the nucleus attracts electrons
• does not effect valence electrons if other energy levels w/ electrons block them
• makes atoms smaller becuz of this^^^
• increases across period and group

Question 30

Direction of group and period

Answer 30

• group: vertical

- period horizontal

Question 31

Trend: Decreases group, increases period

Answer 31

• Ionization energy

- Electronegativity

Question 32

Trend:Increases group, decreases period

Answer 32

• Atomic size

- Ionic size