The Periodic Table

Question 1

What is the periodic table of the elements?

Answer 1

it organizes the elements according to their atomic numbers and reveals a pattern of similar chemical and physical properties among elements.

Question 2

What are the rows of the table called?

Answer 2

Periods, they are based on the same principal energy level n

Question 3

What are the groups of the table?

Answer 3

They are the columns, elements in the same group have the same valence shell electron configuration.

Question 4

What classifies metals?

Answer 4

They are shiny (lustrous) conduct electricity well, and are malleable and ductile. Metals are found on the left side and middle of the table.

Question 5

What are nonmetals?

Answer 5

they are dull, poor conductors of electricity, and are brittle. Non-metals are found on the right side of the periodic table.

Question 6

What are metalloids (semimetals)?

Answer 6

possess characteristics of both metals and nonmetals and are found in a stair-step pattern starting with boron (B).

Question 7

What is the effective nuclear charge (Zeff)?

Answer 7

it is the net positive charge experienced by electrons in the valence shell and forms the foundation for all periodic trends. It tends to increase from left to right across a period, with little change in value from top to bottom in a group.

Question 8

What is the atomic radius?

Answer 8

decreases form left to right across a period and increases from top to bottom in a group.

Question 9

What is the ionic radius?

Answer 9

is the size of a charged species,. The largest nonmetallic Ionic radii and the smallest metallic ionic radii exist at the metalloid boundary. Cations are generally smaller than their corresponding neutral atom while anions are generally larger.

Question 10

What i ionization energy?

Answer 10

It is the amount of energy necessary to remove and electron from the valence shell of a gaseous species; it increases form left to right across a period and decreases form top to bottom in a group. The energy to remove the first is called first ionization energy. The energy is called second and so on.

Question 11

What is electron affinity?

Answer 11

It is the amount of energy released when a gaseous species gains an electron in its valence shell; it increase from left to right across a period and decrease from top to bottom in a group.

Question 12

What is electronegativity?

Answer 12

It is a measure of the attractive force of the nucleus for electrons within a bond; it increases from left to right across a period and decrease form top to bottom in a group.

Question 13

What are the the alkali metals?

Answer 13

typically take on an oxidation state of 1+ and prefer to lose and electron to achieve a noble gas-like configuration; they and the alkaline earth metals are the most reactive of all metals. Group 1 in table. Reacts well with nonmetals, especially halogens.

Question 14

What are the alkaline earth metals?

Answer 14

Take on an oxidation state of +2 and can lose two electrons to achieve noble gas-like configurations. Group 2 on table.

Question 15

What are Chalcogens?

Answer 15

they take on an oxidation state of -2 or +6 (depending on wether they are nonmetals or metals, respectively) in order to achieve noble gas configuration. Group 16. Crucial for biological functions.

Question 16

What are halogens?

Answer 16

typically take on an oxidation state of -1 and prefer to gain an electron to achieve noble gas-like configurations; these nonmetals have the highest electro negativities.
Group 17. Usually found as halides (ion form) or diatomic molecules. highly reactive nonmetals due to having 7 valence electrons.

Question 17

What are noble gases?

Answer 17

They have fully filled valence shell in their standard state and prefer not to give up or take on additional electrons; they have very high ionization energies and (for He, Ne, and Ar), virtually nonexistent electro negativities and electron affinities. Minimal reactivity, low boiling points.

Question 18

What are transition metals?

Answer 18

They are unique because they take on multiple oxidation states, which explains their ability to form colorful complexes with nonmetals in solution and their utility in certain biological systems.

Question 19

What is the periodic law?

Answer 19

the chemical and physical properties of the elements are dependent, in a periodic way, upon their atomic numbers.

Question 20

What are the A elements?

Answer 20

They are known as the representative elements and include groups IA through VIIIA. The elements in these groups have their valence electrons in the orbitals of either s or p subshells.

Question 21

What are the B elements?

Answer 21

They are known as the non-representative elements and include both the transition elements, which have their valence electrons in the s and d subshells and the lanthanide and actinide series, which have valence electrons in the s and f subshells.

Question 22

What metal is not a solid?

Answer 22

Mercury

Question 23

Which metal is less dense than water?

Answer 23

Litium

Question 24

What are active metals?

Answer 24

Elements that have such low ionization, meaning they do not exist naturally in their neutral forms, they are always found as ionic.

Question 25

Which element is the largest, least electronegative, lowest ionization energy, least exothermic electron affinity.

Answer 25

Cs

Question 26

Which element is the smallest, most electronegative, highest ionization energy, most exothermic electron affinity.

Answer 26

F

Question 27

When you go from left to right on a periodic table..?

Answer 27

• atomic radius decrease
• ionization energy increases
• electron affinity increases
• electronegativity increases

Question 28

When you go form top to bottom on the periodic table..?

Answer 28

• atomic radius increase
• ionization energy decrease
• electron affinity decrease
• electronegativity decrease

Question 29

What are the pairs of complementary colors?

Answer 29

-Cyan/red, green/magenta, blue/yellow .