Unit 3 🖊️

Question 1

What people classified the periodic table using atomic mass?

Answer 1

Dobenreigner, Mendeleev, Newlands

Question 2

Who classified the periodic table using atomic number?

Answer 2

Mosely

Question 3

Describe the relationship between electron configuration and the groups and columns of the periodic table

Answer 3

Elements in the same group have the same number of electrons in their outermost shell, leading to similar valence shell electronic configuration

Question 4

What is the Atomic Radius trend?

Answer 4

1/2 distance between the nuclei of 2 atoms of the same element.
Smallest: He
Largest: Fr

Question 5

What is the Electronegativity trend?

Answer 5

The ability of an atom to attract electrons (not including Noble Gases)
Smallest: Fr
Largest: F

Question 6

What is the Ionization Energy trend?

Answer 6

The energy required to remove an electron from an atom
Smallest: Fr
Largest: He

Question 7

What is the Ionic Radius trend?

Answer 7

1/2 distance between the nuclei of charged atoms; Cation<Parent<Anion
Smallest: (+) charge
Largest: (-) charge

Question 8

Describe Electron Affinity

Answer 8

Energy needed to add an electron to a neutral atom (opposite of Ionization Energy)

Question 9

Describe the Electron Shielding Effect

Answer 9

As you go down a group, energy levels are filled with e- generating a (-) charge shield from the nucleus

Question 10

Describe Effective Nuclear Charge

Answer 10

As you go from left to right across the periodic table, the more protons in the nucleus; cause electrons to pair up in orbitals

Question 11

Who believed that physical and chemical properties repeated in an orderly way

Answer 11

Mendeleev

Question 12

Who discovered the periodic law?

Answer 12

Mosely

Question 13

who’s periodic table was meant to show electron configurations?

Answer 13

Mosely

Question 14

What elements did Mendeleev predict?

Answer 14

Gallium, Scandium, and Germanium

Question 15

Who suggested that the properties of an element are related to its atomic mass?

Answer 15

Dobenreigner

Question 16

Who classified elements into triads?

Answer 16

Dobenreigner

Question 17

How many valence electrons are in each main group of the periodic table?

Answer 17

Alkali metals: 1
Alkali Earth metals: 2
Transition metals: 1-2
Group 13: 3
Group 14: 4
Pnictogens: 5
Chalcogens: 6
Halogens: 7
Noble gases: 8

Question 18

reacts vigorously with H20

Answer 18

Alkali Metals

Question 19

Reacts vigorously with O

Answer 19

Alkali Earth metals

Question 20

What group has -4 or +4 charges; -3 charges?

Answer 20

1. Group 14
2. Pnictogens

Question 21

What Periodic group is used as catalysts in petroleum production?

Answer 21

Lanthanides and Actinides

Question 22

What periodic table group is mostly non-reactive?

Answer 22

Transition Metals

Question 23

What periodic group is used as catalysts?

Answer 23

Transition metals

Question 24

What periodic group was formed by accident?

Answer 24

Chalcogens

Question 25

Inert

Answer 25

Noble Gases

Question 26

Form acidic compounds

Answer 26

Halogens

Question 27

Define Valence Electrons

Answer 27

Electrons in the outermost shell of an atom that can be lost, gained, or shared (S and P orbitals only)

Question 28

What block is each group a part of?

Answer 28

Alkali Metals- s Alkali Earth Metals- s Transition Metals- d Group 13- p Group 14-p Pnictogens- p Chalcogens- p Halogens- p Noble Gases- p

Question 29

What is a periodic trend

Answer 29

Specific patterns that are present in the periodic table that illustrate different aspects of a certain element including its size and electronic properties.

Question 30

Explain why atoms form chemical bonds and distinguish between ionic and covalent bonding

Answer 30

1. Chemical bonds happen because every atom wants to be stable; many atoms become stable by having 8 electrons or filling their valence shell with electrons Covalent- electrons are SHARED Ionic- electrons are completely TRANSFERRED

Question 31

As you go down a group on the periodic table, atoms get what?

Answer 31

Bigger

Question 32

True or false: the electron shield is generated as you go down the groups of the periodic table

Answer 32

TRUE

Question 33

The nuclear effect means...

Answer 33

The greater p+ in the nucleus, the more electrons will pair up in orbitals

Question 34

Describe cations and anions

Answer 34

A cation has a net positive electrical charge, which means it has more protons than electrons. An anion has a net negative electrical charge, which means it has more electrons than protons. ANIONS ARE ALWAYS LARGER THAN CATIONS

Question 35

Positive or negative: Cation

Answer 35

Positive

Question 36

Positive or negative: Anion

Answer 36

Negative

Question 37

Why is Helium smaller than Hydrogen?

Answer 37

electron configuration. Helium holds electrons closer to the nucleus.