Periodic Table Unit

Question 1

What happens to ionization energy as it goes across a period?

Answer 1

It increases.

Question 2

Who was the first to publish the periodic table of elements?

Answer 2

Dmitri Mendeleev

Question 3

How did he group the elements?

Answer 3

In columns by similar properties in order of increasing mass.

Question 4

How is the modern periodic table organized?

Answer 4

In the modern periodic table, elements are arranged in order of increasing atomic number. elements with similar properties are in the same column.

Question 5

What determines the chemical properties of an element?

Answer 5

The number of valence electrons.

Question 6

What are electron dot diagrams?

Answer 6

Uses the symbol of the element and dots to represent the electrons in the outer energy level.

Question 7

What are the characteristics of metals?

Answer 7

They are lustrous (shiny) solids, generally high melting points and densities, malleable (can be shaped), ductile (can be pulled into wires), conductors of heat and electricity, and they lose electrons.

Question 8

what are the characteristics of nonmetals?

Answer 8

They are poor conductors of heat and electricity, often dull and brittle, insulators, and gains electrons.

Question 9

How does distance affect the affinity for electrons?

Answer 9

The shorter the distance between the nucleus and the valence electrons, the more strongly they are held by the atom.

Question 10

What is the relationships between number of electrons and the force holding it?

Answer 10

The more electrons between the nucleus and a valence electron, the weaker the force holding it.

Question 11

What is ionization energy?

Answer 11

The energy required to remove an electron from an atom. The greater the attraction the greater the ionization energy, the stronger the attraction between the nucleus and the valence electrons, the harder it is to remove electrons.

Question 12

What are non-metals’ ionization energy/chemical properties?

Answer 12

• They have a strong attraction between nucleus and valence electrons (high ionization energy) difficult to remove electrons
• They have high electronegativity

Question 13

What are metals’ ionization energy/chemical properties?

Answer 13

• They have low ionization energy
• They lose electrons when bonding (metal atoms nuclei have a weak attraction for their valence electrons and so lose them)
• Alkali and alkaline earth metals have little valence electrons so they are the most reactive of the metals
• Metals are found combined in nature

Question 14

What happens to atomic radius as it goes down a group?

Answer 14

It increases.

Question 15

What happens to atomic radius as it goes across a period?

Answer 15

It decreases.

Question 16

What happens to electronegativity as it goes down a group?

Answer 16

It decreases.

Question 17

What happens to electronegativity as it goes across a period?

Answer 17

It increases.

Question 18

What happens to ionization energy as it goes down a group?

Answer 18

It decreases.

Question 19

What is atomic radius?

Answer 19

The distance from the nucleus to the outermost electron.

Question 20

What is electronegativity?

Answer 20

A measure of the tendency of an atom to attract a bonding pair of electrons.

Question 21

Why does atomic radius decrease across a period?

Answer 21

There are a number of protons in the nucleus so the nucleus more strongly attracts its orbital electrons and pulls them closer to it, while electron shielding remains similar.

Question 22

Why does atomic radius increase across a group?

Answer 22

Increasing number of energy levels.

Question 23

Why does electronegativity decrease down a group?

Answer 23

As you move down a group, the radius increases as more electrons shells are added. Since the outer electrons (those involved in bonding) are farther from the nucleus, they will feel the “pull” of the nucleus less. Larger atoms have lower electronegativity.

Question 24

Why does electronegativity increase across a period?

Answer 24

As we move across the period, the effective nuclear charge increases and the atomic size decreases.

Question 25

Why does ionization energy increase across a period?

Answer 25

The nuclear charge of the nucleus is increasing, and the atomic radius is decreasing. These two things increase the pull on the electrons from the nucleus, which makes it require more energy to remove an electron.

Question 26

Why does ionization energy decrease down a group?

Answer 26

Since there are new layers being added the valence electrons are farther from the nucleus and therefore the nucleus has a weaker hold on those electrons so they are easier to remove (less energy).

Question 27

What happens when you read down a group?

Answer 27

The valence electrons are further and further away from the nucleus, valence electrons are removed more easily.

Question 28

What happens to ionization energy as you move down a group?

Answer 28

It decreases.

Question 29

What is the general level of electronegativity of metals?

Answer 29

They have weak attraction for their valence electrons, so they have low electronegativity.

Question 30

What happens when metals lose their valence electrons?

Answer 30

The ion produced is smaller than the original atom.

Question 31

What happens when a nonmetal atom becomes an ion?

Answer 31

It gains electrons, so the radius increases, making it bigger than the original atom.

Question 32

What are monatomic elements?

Answer 32

Elements that only contain one atom. Noble gasses.

Question 33

What are diatomic elements?

Answer 33

H2, N2, O2, F2, Cl2, Br2, I2 - HONCLBRIF

Question 34

What are the elements phases at STP?

Answer 34

Most are solid, mercury and bromine are liquid, and the noble gases plus hydrogen oxygen nitrogen chlorine and fluoride are gases. HONCLF

Question 35

What are monatomic gases?

Answer 35

Single atoms not bonded to each other (noble gasses).

Question 36

Which element has the most metallic character and which has the most nonmetallic character?

Answer 36

Francium has the most metallic character and Fluorine has the most nonmetallic character.

Question 37

What happens to metallic character as we read down and to the left of the table?

Answer 37

It increases.

Question 38

What happens to metallic character as we read up and to the right of the periodic table?

Answer 38

It decreases.

Question 39

What happens to nonmetallic character as we read down and to the left of the table?

Answer 39

It decreases.

Question 40

What happens to nonmetallic character as we read up and to the right of the periodic table?

Answer 40

It increases.

Question 41

What is metallic character?

Answer 41

Metallic character refers to the level of reactivity of a metal. Metals tend to lose electrons in chemical reactions, as indicated by their low ionization energies.