Barsam's Chemistry Chapter 4 Review

Barsam's Chemistry Chapter 4 Review

By Chelsea McBride

Metals, Nonmetals and Metalloids

Some text here about the topic of discussion

The periodic Table is broken up into three sections

• Metals 

• Nonmetals

• Metalloids

​

Periodic Table

Multiple Choice

Oxygen is a ....

• Metal

• Nonmetal

• Metalloid

Multiple Choice

Silicon is a...

• Metal

• Nonmetal

• Metalloid

Multiple Choice

Zircon is a...

• Metal

• Nonmetal

• Metalloid

is a characteristic of a substance that can be observed or measured without changing the identity of the substance

​

Physical Properties

Multiple Choice

Which of the following is not a physical property?

• Luster

• Malleablility

• Conductivity

• All of them ARE physical properties

substances that have the physical properties of luster, conductivity, malleability, and ductility; most of the elements and often seen in solid form.​

​

​Some text here about the topic of discussion.

Metals

Multiple Choice

In what part of the periodic table do you find metals?

• Most of the middle and left side of the periodic table

• The top right side of the periodic table

• Most of the middle and right side of the periodic table

• Along the staircase on the periodic table

​Some text here about the topic of discussion.

​

• ​Shiny luster

• Malleable

• ​Good conductors

• ​Ductile

• ​High density

Metal Physical Properties

​

Multiple Choice

Which of the following is NOT one of the key physical properties for metals?

• Shiny

• Good Conductor

• Dull

• Malleable

substances that have the physical properties of being dull, insulators, and brittle; may appear in all three states of matter

​

Nonmetals

Multiple Choice

Where are nonmetals located on the periodic table?

• Most of the middle and left side of the periodic table

• The top right side of the periodic table and hydrogen

• Most of the middle and right side of the periodic table

• Along the staircase on the periodic table

• Dull

• ​Brittle

• Not malleable

• Insulator

• Not ductile​

​

​Some text here about the topic of discussion.

Nonmetal Physical Properties

​

Multiple Choice

Which of the following is a main physical properties of nonmetals?

• Dull

• Malleable

• Good Conductor

• All of them

Elements that have properties of both metals and nonmetals; found between metals and nonmetals on periodic table​

Metalloids

Multiple Choice

Where are the metalloids located on the periodic table?

• Most of the middle and left side of the periodic table

• The top right side of the periodic table and hydrogen

• Most of the middle and right side of the periodic table

• Along the staircase on the periodic table

• ​Typically solids

• Can be shiny or dull

• Can be malleable

• Can be ductile

• Can be brittle

• Good semiconductor​

Metalloid Physical Properties

Multiple Choice

Which of the following is a key characteristic of metalloids?

• Used as semiconductors

• Ductile

• Insulator

• Malleable

Periodic Table

By Craig LaPerriere

Multiple Choice

What is a group

• Up and down row on the table

• Up and down column on the table

• Side to side row on table

• Side to side column on the table

Multiple Choice

What is a period?

• Up and down row on the table

• Up and down column on the table

• Side to side row on table

• Side to side column on the table

Multiple Choice

What group is carbon in?

• 1

• 2

• 13

• 14

• 15

Multiple Choice

Where are the transition metals located

• Left side of table

• Top of table

• middle of table

• right side of table

Multiple Choice

Which is a transition metal?

• Aluminum

• Calcium

• Sodium

• Chromium

Multiple Choice

Which element is a Transition Metal?

• Strontium

• Silicon

• Titanium

• Cessium

Multiple Choice

Which element is a Halogen?

• Argon

• Iodine

• Calcium

• Sodium

Multiple Choice

Why are halogens so reactive

• Need 7 valence electrons

• Need to lose 1 electron to be stable

• Need to add 1 electron to be stable

• They are super large atoms

Multiple Choice

Which element is a Noble Gas?

• Neon

• Chlorine

• Sodium

• Phosphorus

Multiple Choice

Why are noble gases not reactive

• Too few electrons

• Too many electrons

• They have a full set of electrons

• They need more electrons

Multiple Choice

Group 18

• Alkali Metals

• Alkaline Earth Metals

• Rare Earth Metals

• Noble Gases

• Halogens

Multiple Choice

Group 1

• Alkali Metals

• Alkaline Earth Metals

• Rare Earth Metals

• Noble Gases

• Halogens

Multiple Choice

Group 17

• Alkali Metals

• Alkaline Earth Metals

• Rare Earth Metals

• Noble Gases

• Halogens

​Valence electrons:

​The electrons in an atom’s outermost orbitals; determine the chemical properties of an element.​

-Each group of representative elements (1,2, 13-18) have an assigned amount of valence electrons.

Fill in the Blank

How many valence electrons does Magnesium have?

Multiple Choice

Noble Gases have how many valence electrons

• 1

• 2

• 6

• 8

Fill in the Blank

How many valence electrons does Bromine have?

Multiple Choice

Alkali Metals have how many valence electrons

• 1

• 2

• 6

• 8

Fill in the Blank

How many valence electrons does Sodium have?

Fill in the Blank

How many valence electrons does Aluminum have?

Fill in the Blank

How many valence electrons does Nitrogen have

​Why do elements form ions of a certain charge?

​Everybody wants the electron configuration of a noble gas! Its the lowest energy state :)

Multiple Choice

When Halogens form ions, what is the charge of the ion?

• 7 +

• 7 -

• 1 -

• 1 +

Multiple Choice

What charge of ion will Sodium form?

• 1-

• 1+

• 7-

• 2-

Multiple Choice

When Magnesium forms an ion, what charge will that ion have?

• +1

• +2

• -2

• -1

Multiple Choice

What charge of ion will Aluminum form?

• 1-

• 2+

• 3-

• 3+

Metals, Metalloids, and Nonmetals

• The periodic table is divided into 3 types of chemicals

• They are in alphabetical order: 1. Metal, 2. Metalloid, 3. Nonmetal

• Metals are the largest group

• Metalloids are the smallest group between metals and nonmetals.

Multiple Choice

Metals are on the:

• Left side

• Right Side

• Stairstep

Multiple Choice

Nonmetals are on the:

• Left side

• Right Side

• Stairstep

Multiple Choice

A student is studying a mystery substance. It breaks easily. It has a very dull luster. It doesn't conduct any electricity. What is the most likely substance this is?

• Metal

• Metalloid

• Nonmetal

Multiple Choice

The same student works with a new substance. He concludes it conducts electricity very well. It has a very shiny luster. When he hammers it, it simply dents and flattens. What is the most likely substance type?

• Metal

• Metalloid

• Nonmetal

Multiple Choice

The third substance the student works with is a little brittle. It is just a little shiny. When he tries to conduct electricity through it at first, it doesn't conduct, but upon heating up, it does start to allow electrons to flow. What is the most likely substance type?

• Metal

• Metalloid

• Nonmetal

Multiple Choice

Order the following elements in terms of increasing electronegativity

F, At, I, Cl,

• F, Cl At, I

• At, F, Cl, I

• At, I Cl, F

• F, Cl, I , At

Multiple Choice

Which accurately describes nonmetals?

• Both malleable and ductile
• Often used in computer parts
• Poor conductors of electricity
• Always solid at room temperature

Multiple Choice

Which group on the periodic table is the most reactive Metals?

• Alkaline-earth metals - Group 2
• Alkali metals - Group 1
• Transition metals - Group 3-7
• Halogens - Group 17

Multiple Choice

Which group of elements is inert?

• Alkaline metals - Group 1
• Alkaline-earth metals - Group 2
• Transition metals Groups 3-8
• Noble Gases - Group 18

Multiple Choice

Which group includes some of the most familiar elements like nickel, iron, and copper?

• Inner transition metals
• Transition metals
• Halogens
• Noble gases

Multiple Choice

Which pair of elements would have similar properties due to the position in the periodic table?

• Calcium (Ca), Helium (He)
• Copper (Cu), Gold (Au)
• Lithium (Li), Beryllium (Be)
• Aluminum (Al), Zinc (Zn)

Periodic Trends

Review

Increasing Atomic Radius

Increasing Atomic Radius

Cation Radius < Neutral < Anion Radius

Increasing Ionization Energy

Increasing Ionization Energy

Decreasing Electronegativity

Increasing Electronegativity

Electronegativity

• Increases as you move across the periodic table.

• Group 1 and 2 metals are the least electronegative elements and tend to lose electrons when forming ions.

• Nitrogen, oxygen, and halogens are the most electronegative and strongly attract electrons when in compounds.

• Decreases or stays the same moving down a group.

Multiple Choice

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

• decreases, increases

• increases, decreases

Multiple Choice

Which element has a higer Elecronegativity?

• Sulfur

• Oxygen

• Nitrogen

• Francium

Multiple Choice

Most elements on the periodic table are classified as __________.

• Metals
• Non-Metals
• Metaloids
• Gases

Multiple Choice

Order the following elements in terms of increasing atomic radii

Ca, Sr, Be , Mg

• Ca, Mg, Be, Sr

• Be, Mg, Ca, Sr

• Sr, Ca, Mg, Be

• Mg, Ca, Sr, Be

Multiple Choice

Order the following elements in terms of increasing electronegativity

Al, Mg, P, Cl

• Mg, Al, Cl, P

• Cl, P, Mg, Al

• Cl, P, Al, Mg

• Mg, Al, P, Cl

Ionization Energy

• The energy required to remove one electron from the outer shell of a neutral atom.

• This is the energy needed to form an ion.

• When ionization energy is high it is harder to remove that electron.

Multiple Choice

What is ionization energy?

• The energy required to remove an electron from a neutral atom

• The energy required to add an electron to a neutral atom

• The energy required to break a chemical bond

• The energy required to form a chemical bond

Multiple Choice

Order the following element in terms of increasing Atomic Radii

Si, Na, S, Mg

• S, Si, Mg, Na

• Na, Mg, Si, S

• S, Si, Mg, Na

• Na, Mg, S , Si

Multiple Choice

Which has the greater Electronegativity: 
N or C?

• C
• N

Atomic and Ionic Radii

Understanding the size of atoms and ions

Atomic and Ionic Radii

• The table of atomic radii shows groups and periods of elements.
• Atomic radius is measured in picometers (pm) in scientific notation.
• The smallest atomic radius is 31 pm (He) and the largest is 225 pm (Fr).
• Within a period, atomic radii generally decrease as the atomic number increases.
• Exceptions to this trend include noble gases and transition metals.

Multiple Choice

What is the general trend of atomic radii within a period?

• Atomic radii generally increase as the atomic number increases.

• Atomic radii generally decrease as the atomic number increases.

• Atomic radii remain constant within a period.

• Atomic radii are not affected by the atomic number.

Atomic Radii Trend

Trivia: Did you know that atomic radii generally decrease as the atomic number increases within a period? This means that atoms become smaller as you move from left to right across a period on the periodic table. It's an interesting trend to observe!

Trends in Atomic Radii

• Within a period: Atomic radii generally decrease from left to right across a period due to increasing nuclear charge and stronger attraction between the electrons and the nucleus.
• Within a group: Atomic radii generally increase as the atomic number increases due to the addition of new energy levels or shells.
• Exceptions: Transition metals have smaller atomic radii than expected due to the presence of d-block electrons.

Multiple Choice

Why do atomic radii generally decrease from left to right across a period?

• Due to the addition of new energy levels or shells

• Due to increasing nuclear charge and stronger attraction between the electrons and the nucleus

• Due to the presence of d-block electrons

• Due to the increasing atomic number

Atomic Radii Trend

Trivia: Atomic radii generally decrease from left to right across a period due to increasing nuclear charge and stronger attraction between the electrons and the nucleus. This trend is known as the electronegativity trend. It affects various properties of elements, such as their reactivity and ability to form chemical bonds.

• Smaller atomic radii result in higher ionization energy and electronegativity.
• The trend is reversed when moving down a group, as new energy levels or shells are added.

Atomic and Ionic Radii

• Atomic radii decrease from left to right across a period and increase from top to bottom within a group.
• Ionic radii of elements in groups 1 and 2 decrease as the group number increases.

Multiple Choice

Which statement is true about atomic radii?

• Atomic radii increase from left to right across a period

• Atomic radii increase from top to bottom within a group

• Atomic radii decrease from left to right across a period

• Atomic radii decrease from top to bottom within a group

Atomic Radii

Trivia: Atomic radii decrease from left to right across a period. This means that as you move from left to right across the periodic table, the size of the atoms decreases. However, atomic radii increase from top to bottom within a group. So, atoms get larger as you move down a group. This trend is due to the increasing number of protons and electrons in the atoms.

Atomic and Ionic Radii

• Atomic Radius within a Period: Generally decreases as atomic number increases due to increased positive charge pulling outermost electrons closer to the nucleus.
• Exceptions: Antimony (Sb) and tellurium (Te) in period 5, and bismuth (Bi) and polonium (Po) in period 6.
• Atomic Radius within a Group: Generally increases as atomic number increases due to larger orbitals and shielding by inner electrons.
• Charge of Ion: Same as the element's group number.

Multiple Choice

What is the general trend of atomic radius within a period?

• Increases as atomic number increases

• Decreases as atomic number increases

• Remains constant within a period

• Depends on the element's group number

Atomic Radius Trend

Trivia: Did you know that the atomic radius decreases as the atomic number increases within a period? This means that atoms become smaller as you move from left to right across a period on the periodic table. It's all about the increasing positive charge in the nucleus attracting the electrons more strongly, making the atomic radius smaller.

Oxidation State Practice

Electronegativity and Chemical Bonds

Predicting bond types

By knowing whether the two elements in a bond are metal or nonmetal you can predict the bond type.

Predicting bond types

As you can see if one element is a metal and one is a nonmetal it will usually form an ionic bond.

Predicting bond types

As you can see if one element is a nonmetal and the other is a nonmetal it will usually form a covalent bond.

The pink diagonal line you see is called the stair-step.

The purple left of the stair-step are metals (with the exception of hydrogen)

The green right of the stair-step are nonmetals and included hydrogen

The pink colored elements that make up the stair-step are metalloids or semi-metals

Don't worry about the value. We want the absolute value (always positive) of the difference.

Multiple Choice

Determine the type of bond that exists between the following pairs of atoms: B & P

• Ionic Bond

• Covalent

Multiple Choice

Determine the type of bond that exists between the following pairs of atoms: Li & O

• Ionic Bond

• Covalent

Multiple Choice

Determine the type of bond that exists between the following pairs of atoms: C & Na

• Ionic Bond

• Covalent

Multiple Choice

Predict the bond types of the following elements: Mg and F

• Ionic

• Nonpolar Covalent

• Polar Covalent

Multiple Choice

Predict the bond types of the following elements: Zn and Cl

• Ionic

• Nonpolar Covalent

• Polar Covalent

Multiple Choice

Predict the bond types of the following elements: N and I

• Ionic

• Nonpolar Covalent

• Polar Covalent

Multiple Choice

Predict the bond types of the following elements: B and Si

• Ionic

• Nonpolar Covalent

• Polar Covalent

Multiple Choice

As you move down a group, electron affinity

• increases

• decreases

Multiple Choice

As you move left to right across a period, electron affinity

• increases

• decreases

Multiple Choice

Which of these has a greater need for electrons?

• Li

• Be

Multiple Choice

Which of these has a greater need for electrons?

• Ca

• Ba

Multiple Choice

Which of these has a greater electron affinity?

• Na

• K

Multiple Choice

Which of these has a greater electron affinity?

• P

• Cl

Multiple Choice

Which of these has a greater electron affinity?

• Si

• Cl

Multiple Choice

Which of these has a greater electron affinity?

• Li

• K

Multiple Choice

What's the difference between electronegativity and electron affinity?

• Electronegativity is a measured energy value and electron affinity is a man-made number.
• Electron affinity is a measured energy value and electronegativity is a man-made number.

Multiple Choice

Define electron affinity.

• The energy it takes to add an electron to an atom.
• The energy it takes to remove an electron from an atom.

Multiple Choice

The electron affinity of a metal is positive (endothermic).

• True
• False

Multiple Choice

The electron affinity of a nonmetal is negative (exothermic).

• True
• False

Multiple Choice

Elements closer to the noble gases have stronger attraction for electrons.

• True
• False

Multiple Choice

Which of the following has the least electron affinity?

• oxygen

• potassium

• fluorine

• nitrogen

Multiple Choice

Which of the following has the most electron affinity?

• nitrogen

• phosphorus

• arsenic

• lithium

Multiple Choice

Put these in order of increasing electron affinity:
F, N, B

• B < N < F

• B < F < N

• N < F < B

• F < N < B

Multiple Choice

Put these in order of increasing electron affinity:
Se, S, and O

• Se < S < O

• Se < O < S

• O < S < Se

• S < Se < O

Multiple Choice

Chlorine and Fluorine are both very electronegative, as they are both missing a single electron from their valence energy level.  Why is Fluorine more electronegative than Chlorine? 

• Fluorine has less energy levels.
• Chlorine has more electrons in its outer shell
• Fluorine has more protons.
• None of these

Multiple Choice

Which elements have zero electron affinity?

• metals

• nonmetals

• metalloids

• noble gases

Multiple Choice

Among the following, the species with the highest electron affinity is

• F^-1

• O

• O^-1

• Na⁺¹

Multiple Choice

The electronic configuration of four elements is given below. Arrange these elements in the correct order of magnitude of their electron affinity

i. 2s²2p⁵ ii. 3s²3p⁵ iii. 2s²2p⁴ iv. 3s²3p4

• 
  $$i<ii<iii<iv$$

• $$ii<i<iv<iii$$

• $$iii<iv<ii<i$$

• $$iii<iv<i<ii$$

Multiple Choice

Electron affinity is expressed in _____.

• KJ mol^-1

• eV

• pm

• JK^-1

Multiple Choice

When we add electron to the neutral atom, it will become a / an _____.

• Cation

• α – particle

• Anion

• β – particle

Multiple Choice

The elements have almost zero electron affinity are _____.

• Be & B

• N & O

• Na & N

• Be & N

Multiple Choice

In each period, _____ has high electron affinity.

• halogen

• alkaline earth metal

• alkali metal

• chalcogen

Multiple Choice

Which of the given atoms has the lowest electron affinity?

• Sr

• Be

• Ca

• Ra

Multiple Choice

The formation of the oxide ion O2-(g) requires first an exothermic and then an endothermic step - as shown below:

O(g) + e- ====> O-(g) ; ΔH0= -142 kJ mol-1

O-(g) + e- ====> O2-(g) ; ΔH0= +844 kJ mol-1

This is because?

• oxygen is more electronegative

• oxygen has high electron affinity

• O ^- ion will tend to resist the addition of another electron

• O ^- ion has comparatively larger size than oxygen atom

Multiple Choice

The electron affinity values (in kJ mol-1) of three halogens X, Y and Z are respectively -349, -333 and -325. Then X, Y and Z respectively are:

• F, Cl and Br

• Cl, F and Br

• Cl, Br and F

• Br, Cl and F

Rule 1: For pure elements (unbonded or only bonded with itself), each atom has an oxidation number of zero. 

• The oxidation state of Na in Na is zero (0)

• The oxidation state of H in H₂ is zero (0)

Multiple Choice

What is the oxidation state of S in S₈?

• -2

• -16

• 0

• 2

Rule 2: Monatomic (single) ions have oxidation numbers equal to their charge.

• The oxidation state of Na⁺ is +1

• The oxidation state of S^2- is -2

Rule 3: Oxygen’s oxidation number is -2 except when in peroxides (such as H₂0₂), where it is -1.

• A peroxide is a compound containing 2 +1 cations and 2 oxygen ions

• The oxidation state of O in Na₂O₂ (sodium peroxide) is -1

Multiple Choice

What is the oxidation state of C in CO?

• +4

• -4

• +2

• -2

Rule 4: Hydrogen’s oxidation number is +1, except for when bonded to metals as the hydride ion forming ionic compounds. 

• The oxidation state of H in H₂O is +1

• The oxidation state of H in NaH is -1

Multiple Choice

What is the oxidation state of N in HNO₃?

• +5

• -3

• -1

• -5

Rule 5: Fluorine (F) has an oxidation number of -1 in ALL of its compounds 

• NO EXCEPTIONS!!

Rule 6: Halogens (Cl, Br, I) have negative oxidation numbers when they form halide compounds. When combined with oxygen, they have positive numbers, except for F. 

• The oxidation state of Cl in HCl is -1

• The oxidation state of Cl in HClO₃ is +5

Multiple Choice

What is the oxidation state of Br in HBrO₄?

• -1

• -7

• +7

• -5

Rule 7: In a neutral atom or molecule, the sum of the oxidation numbers must be 0. In a polyatomic ion, the sum of the oxidation numbers of all the atoms in the ion must equal the charge on the ion 

• Use Table E to check charges of polyatomic ions

Multiple Choice

What is the oxidation state of Cr in CrO₄^2- ?

• +6

• +2

• -2

• +8

Multiple Choice

What is the oxidation number of Mn in MnO₄^- ?

• -2

• +2

• +7

• +8

Multiple Choice

What is oxidation number of P in K₃PO₄?

• -2

• -1

• +1

• +5

Multiple Choice

What is oxidation number of K in K₃PO₄?

• -2

• -1

• +1

• +5

Multiple Choice

What is the oxidation number of Cl in FeCl₃?

• -3

• -1

• +1

• +3

Multiple Choice

What is the oxidation number of Fe in FeCl₃?

• -3

• -2

• +2

• +3

Multiple Choice

What is the oxidation state of H in H₂?

• 0

• +1

• -1

• -2

Poll

How are you feeling with oxidation states as of now?

• Really good! 10/10

• Pretty solid, could maybe use some more practice

• Eh, still kinda tricky

• Very confused and need more help here!