Electronic Structure and Periodicity

Question 1

Who created the initial draft of periodic table in the mid-19th century?

Answer 1

Dmitry I. Mendeleev

Question 2

The rows are called _______, and they are numbered from 1 to 7. This is also categorized horizontally.

Answer 2

Periods

Question 3

The elements are stacked so that elements with similar chemical properties form vertical columns, called ________, numbered from 1 to 18.

Answer 3

Groups

Question 4

The group 1 in the periodic table is consist of _______.

Answer 4

Alkali Metals

Question 5

The group 2 in the periodic table is consist of _______.

Answer 5

Alkaline Earth Metals

Question 6

The group 3-12 in the periodic table is consist of _______.

Answer 6

Transition Metals

Question 7

The group 13 in the periodic table is consist of _______.

Answer 7

Boron Group (triels)

Question 8

The group 14 in the periodic table is consist of _______.

Answer 8

Carbon Group (tetrels)

Question 9

The group 15 in the periodic table is consist of _______.

Answer 9

Pnictogens or Nitrogen group

Question 10

The group 16 in the periodic table is consist of _______.

Answer 10

Chalcogens or Oxygen group

Question 11

The group 17 in the periodic table is consist of _______.

Answer 11

Halogens

Question 12

The group 18 in the periodic table is consist of _______.

Answer 12

Noble gases

Question 13

These elements are highly conductive elements to heat and electricity, usually solid, malleable, and ductile.

Answer 13

Metals

Question 14

Elements that are poor in conduction of heat and electricity, very brittle, and cannot be rolled into wires or pounded into sheets. Some can exist as either solid or gas at room temperature.

Answer 14

Non-metals

Question 15

Elements found along the stair-step line that distinguish metals from non-metals and have properties of both metals and non-metals.

Answer 15

Metalloids

Question 16

Includes the active metals in the two (2) columns on the extreme left of the periodic table and the metals, metalloids, and nonmetals in the six (6) columns on the far right.

Answer 16

Main-group elements

Question 17

_______________ are more electronegative than the main group metals and, therefore, more likely to form covalent compounds.

Answer 17

Transition metals

Question 18

Located at the bottom of the table, they are sometimes known as the inner transition metals because they have atomic numbers that fall between the first and second elements in the last two (2) rows of the transition metals.

Answer 18

Actinides and Lanthanides

Question 19

Also known as “ore formers” are members of this group that show increasing metal character as the atomic number increases.

Answer 19

Chalcogens

Question 20

Also known as “salt formers” these elements exist as diatomic molecules in elemental states that are highly reactive and readily combine with most elements.

Answer 20

Halogens

Question 21

Refers to inert gasses, which have an oxidation state of 0, contain a maximum number of electrons in their outer shell, making them stable.

Answer 21

Noble gases

Question 22

The main group elements are the most abundant in the universe and are often called ___________________.

Answer 22

Representative elements

Question 23

Properties of s-block elements

Answer 23

1. The oxidation state of Group 1 elements, the alkali metals, is +1. The Group 2 elements, alkaline earth metals’ oxidation number is +2.
2. These elements are very reactive except Helium.
3. The s-block metals are soft and have low melting and boiling points.
4. The metals in the s-block react to form basic oxides, hydrides, and hydroxides.

Question 24

Groups that are located at the p-block in the periodic table

Answer 24

Group 13 - Icosagens
Group 14 - Crytsallogens
Group 15 - Pnictogens
Group 16 - Chalcogens
Group 17 - Halogens
Group 18 - Noble gases

Question 25

Properties of p-block elements

Answer 25

1. The oxidation states of p-block metals vary but are generally dependent on the electrons in the p-orbital. The noble gases of Group 18 have oxidation states equal to zero (0) because they are stable.
2. The p-block elements comprise non-metals, metalloids, and metals; thus, their properties vary.
3. The non-metals F, Cl, Br, and I form ionic compounds in the p-block.

Question 26

Tendency of an electron to bond.

Answer 26

Electronegativity

Question 27

The electronegativity of electrons (1) __________ from left to right along a (2) __________ and (3) _________ from top to bottom along a (4) ____________.

Answer 27

1. Increases
2. Period
3. Decreases
4. Column or group

Question 28

The energy needed to remove an electron from an atom.

Answer 28

Ionization Energy

Question 29

The Ionization energy of electrons (1) __________ from left to right along a (2) __________ and (3) _________ from top to bottom along a (4) ____________.

Answer 29

1. Increases
2. Period
3. Decreases
4. Column or group

Question 30

The energy released when an electron is added to an atom.

Answer 30

Electron Affinity

Question 31

In electron affinity, the energy is positive when (1) ___________ and (2) __________ when absorbed.

Answer 31

1. Released
2. Negative

Question 32

The electron affinity of electrons increases from (1) ______ to (2) ________ along a period and decreases from (3) _______ to (4) ________ along a column or a group.

Answer 32

1. left
2. right
3. top
4. bottom

Question 33

The farthest extent of the presence of electrons.

Answer 33

Atomic Size/Radius

Question 34

The atomic size or radius of electrons (1) __________ from left to right along a (2) __________ and (3) _________ from top to bottom along a (4) ____________.

Answer 34

1. Decreases
2. Period
3. Increases
4. Column or group

Question 35

Defined as how readily an atom can lose an electron.

Answer 35

Metallic Property

Question 36

The metallic character (1) _________ from (2) _______ to left and (3) _________ from top to (4) __________.

Answer 36

1. Increases
2. Right
3. Increases
4. Bottom