2B2 The Periodic Table

Question 1

What is the periodic table?

Answer 1

A chart of elements arranged by atomic number.

The periodic table organizes elements into rows (periods) and columns (groups) based on their properties.

Question 2

True or False:

The periodic table is arranged by atomic mass.

Answer 2

False

It is arranged by atomic number.

Question 3

What is a group in the periodic table?

Answer 3

A vertical column of elements with similar properties.

Groups are numbered 1 to 18 and elements in the same group have the same number of valence electrons.

Question 4

What is a period in the periodic table?

Answer 4

A horizontal row of elements with increasing atomic number.

As you move across a period, properties like electronegativity and ionization energy generally increase. There are 7 periods in the periodic table.

Question 5

Fill in the blank:

An element consists of atoms that all have the same number of _________.

Answer 5

protons

The number of protons in an atom determines its atomic number and identifies the element on the periodic table.

Question 6

What does the atomic number represent?

Answer 6

The number of protons in an atom’s nucleus.

The atomic number determines the element’s identity and its position in the periodic table.

Question 7

What is the atomic number of carbon?

Answer 7

6

Carbon has 6 protons, so its atomic number is 6.

Question 8

What do you call elements that are good conductors of electricity, malleable and ductile?

Answer 8

Metals

Metals are typically found on the left side and in the center of the periodic table. Examples include iron (Fe) and copper (Cu).

Question 9

True or False:

All metals are solid at room temperature.

Answer 9

False

While most metals are solid at room temperature, mercury (Hg) is a liquid metal.

Question 10

Where are oxygen (O) and carbon (C) located on the periodic table?

Answer 10

On the right side as nonmetals.

Nonmetals are poor conductors and are essential for life processes, like respiration and photosynthesis.

Question 11

Where are metals located on the periodic table?

Answer 11

On the left side and center.

Metals are generally conductive, malleable, and shiny.

Question 12

Where are nonmetals located on the periodic table?

Answer 12

On the right side.

Nonmetals are typically poor conductors and have higher electronegativity.

Question 13

Where are metalloids located?

Answer 13

Between metals and nonmetals.

Metalloids have mixed properties of metals and nonmetals, such as silicon.

Question 14

Fill in the blank:

Metalloids are also called _______.

Answer 14

Semimetals

Metalloids are used in electronics due to their semi-conductivity.

Question 15

Which element is an example of a metalloid?

Answer 15

Silicon (Si)

Silicon is a metalloid used in semiconductors, bridging the properties of metals and nonmetals.

Question 16

Which group of elements is called the transition metals?

Answer 16

Groups 3–12

These metals are characterized by variable oxidation states and are often used in alloys.

Question 17

What is the symbol for Helium?

Answer 17

He

Helium (He) is a noble gas in Group 18.

Question 18

What is the symbol for Copper?

Answer 18

Cu

Copper (Cu) is a transition metal known for its electrical conductivity.

Question 19

Where are the lanthanides and actinides located?

Answer 19

Below the main periodic table.

These two series of elements, often called the f-block, are placed separately to save space.

Question 20

What are alkali metals?

Answer 20

Group 1 elements.

Alkali metals like lithium (Li) and sodium (Na) are highly reactive and have one electron in their outer shell.

Question 21

What are alkaline earth metals?

Answer 21

Group 2 elements.

Alkaline earth metals like magnesium (Mg) and calcium (Ca) are reactive but less so than alkali metals.

Question 22

True or False:

Transition metals can have more than one oxidation state.

Answer 22

True

Transition metals like iron (Fe) can form different positive ions, such as Fe²⁺ and Fe³⁺.

Question 23

What is the symbol for Calcium?

Answer 23

Ca

Calcium (Ca) is an alkaline earth metal in Group 2.

Question 24

Where are halogens found?

Answer 24

Group 17

Halogens like fluorine (F) and chlorine (Cl) are reactive nonmetals.

Question 25

# Define: Ionization energy

Answer 25

The energy **required** to remove an electron. ## Footnote Ionization energy generally increases across a period and decreases down a group.

Question 26

# True or False: Alkali metals have a **charge** of +2.

Answer 26

False ## Footnote Alkali metals have a charge of +1 due to losing one electron.

Question 27

What type of **bonding** occurs between metals?

Answer 27

Metallic bonding. ## Footnote In metallic bonding, electrons are delocalized and shared freely among atoms.

Question 28

# Fill in the blank: In **ionic bonding**, metals \_\_\_\_\_\_\_ electrons and nonmetals \_\_\_\_\_\_\_ electrons.

Answer 28

lose, gain ## Footnote Metals lose electrons to form positive ions, while nonmetals gain electrons to form negative ions.

Question 29

Where are the most **reactive** elements located?

Answer 29

In the alkali metals and halogens. ## Footnote Alkali metals react vigorously with water, and halogens are highly reactive with metals.

Question 30

You’re an architect choosing materials for a skyscraper. Which **side** of the periodic table would you look at for strong, durable metals?

Answer 30

The center (transition metals). ## Footnote **Transition metals** like steel (an alloy of iron) and titanium (Ti) are used for their strength and resistance to corrosion, perfect for structural materials.

Question 31

What **group** are the halogens in?

Answer 31

Group 17 ## Footnote Halogens, such as fluorine (F) and chlorine (Cl), are very reactive and form salts when combined with metals.

Question 32

# Define Noble gases

Answer 32

**Inert gases** with full outer electron shells. ## Footnote Noble gases like neon (Ne) and argon (Ar) are **stable** and rarely form compounds because their outer electron shells are full.

Question 33

# True or False: **Nonmetals** tend to form positive ions.

Answer 33

False ## Footnote Nonmetals typically form negative ions by gaining electrons.

Question 34

A scientist wants to develop a new, **non-reactive** gas for use in lightbulbs. Which group in the periodic table should he look at?

Answer 34

Group 18 (Noble gases). ## Footnote Noble gases like argon (Ar) are chemically inert, making them ideal for preventing oxidation inside lightbulbs.

Question 35

What is **atomic radius**?

Answer 35

The **distance** from the nucleus to the outermost electron. ## Footnote The atomic radius *reflects* the size of an atom, and it decreases across a period and increases down a group.

Question 36

# Fill in the blank: Elements in **group 1** have the \_\_\_\_\_\_\_\_ atomic radius.

Answer 36

largest ## Footnote Group 1 elements have only one electron in their outermost shell, making them the largest in size.

Question 37

# True or False: Atomic radius **increases** as you move down a group.

Answer 37

True ## Footnote New electron shells are added with each period, increasing the distance between the nucleus and outer electrons.

Question 38

You are comparing two metals for use in electrical wiring. One is in Group 1 and the other in Group 2. Which metal will likely have a **larger** atomic radius?

Answer 38

The group 1 metal. ## Footnote Group 1 elements like lithium (Li) have larger atomic radii because they have fewer protons, so their electrons are less tightly pulled towards the nucleus.

Question 39

What is **ionization energy**?

Answer 39

The energy **required** to remove an electron from an atom. ## Footnote High ionization energy means it is harder to *remove* an electron, like in noble gases.

Question 40

What **happens** to ionization energy as you move across a period?

Answer 40

It increases. ## Footnote As atomic size decreases, electrons are held more tightly, making them harder to remove.

Question 41

# True or False: Ionization energy is **higher** for smaller atoms.

Answer 41

True ## Footnote Smaller atoms have *stronger* attractions between the nucleus and electrons, requiring more energy to remove an electron.

Question 42

Which **element** is more likely to form an ionic bond: lithium (Li) or chlorine (Cl)?

Answer 42

Both are likely, but lithium will **lose** an electron, and chlorine will **gain** one. ## Footnote Lithium, a metal from Group 1, has low ionization energy, making it easy to lose electrons, while chlorine, a nonmetal from Group 17, has high electronegativity, making it eager to gain electrons.

Question 43

# True or False: Electronegativity **decreases** as you move down a group.

Answer 43

True ## Footnote As the atomic radius increases, the nucleus' ability to attract bonding electrons weakens.

Question 44

# Fill in the blank: \_\_\_\_\_\_\_ has the **highest** electronegativity.

Answer 44

Fluorine ## Footnote ***Fluorine*** is the most electronegative element, strongly attracting electrons in chemical bonds.

Question 45

# True or False: The electronegativity of **alkali metals** is high.

Answer 45

False ## Footnote Alkali metals have **low** electronegativity because they easily lose their outer electron, rather than attracting others.

Question 46

A jeweler is looking for a metal that doesn’t **tarnish** easily. Which metal should he use?

Answer 46

Platinum (Pt) or gold (Au). ## Footnote Both platinum and gold are **transition metals** with excellent corrosion resistance, perfect for jewelry that needs to retain its shine.

Question 47

What happens to **metallic bonding** across a period?

Answer 47

It strengthens. ## Footnote As you move across a period, the number of protons increases, leading to stronger attraction between the electrons and the nucleus, which strengthens the metallic bonds.

Question 48

# True or False: Melting points of metals **increase** across a period.

Answer 48

True ## Footnote As metallic bonding becomes stronger, it requires more energy to break the bonds, raising the melting points.

Question 49

What is **reactivity**?

Answer 49

The **ability** of an element to undergo a chemical reaction. ## Footnote Reactivity depends on how *easily* an element can lose or gain electrons.

Question 50

What **determines** an element’s reactivity?

Answer 50

The **number** of valence electrons. ## Footnote Elements with fewer valence electrons (metals) are *generally* more reactive.

Question 51

What happens to reactivity in metals as you go down a **group**?

Answer 51

It increases. ## Footnote Larger atoms lose electrons more easily, making metals more reactive down the group.

Question 52

What happens to reactivity in metals as you go across a **period**?

Answer 52

It decreases. ## Footnote As atomic size decreases, metals hold onto electrons more tightly, lowering reactivity.

Question 53

# True or False: Group 1 metals are **highly reactive**.

Answer 53

True ## Footnote Group 1 metals have one electron in their outer shell, which they lose easily in reactions.

Question 54

What is the reactivity trend for **noble gases**?

Answer 54

They are non-reactive. ## Footnote Noble gases have full electron shells, making them chemically stable.

Question 55

Which group contains the most reactive **nonmetals**?

Answer 55

Group 17 ## Footnote Halogens in Group 17, such as fluorine (F) and chlorine (Cl), are highly reactive.

Question 56

Which group contains the most reactive **metals**?

Answer 56

Group 1 ## Footnote Alkali metals, like lithium (Li) and sodium (Na), are highly reactive, especially with water.

Question 57

# Fill in the blank: Nonmetals **react** by \_\_\_\_\_\_\_\_ electrons.

Answer 57

gaining ## Footnote Nonmetals tend to gain electrons to achieve a *full valence shell*, which makes them more stable.

Question 58

# True or False: Transition metals are **highly reactive** compared to alkali metals.

Answer 58

False ## Footnote Transition metals are **less reactive** than alkali metals. Alkali metals are highly reactive because they easily lose their single valence electron, while transition metals have more stable electron configurations and typically do not lose electrons as easily.

Question 59

How does the reactivity of metals **compare** to nonmetals?

Answer 59

Metals **lose** electrons, nonmetals **gain** them. ## Footnote Metals tend to form positive ions, while nonmetals tend to form negative ions.

Question 60

# Fill in the blank: Alkali metals **react** violently with \_\_\_\_\_\_\_.

Answer 60

water ## Footnote Alkali metals, such as sodium (Na) and potassium (K), react violently with water, producing hydroxides and hydrogen gas. This highly exothermic reaction can generate flames or cause explosions due to the rapid release of energy.