Periodic Trends

Multiple Choice

Coulombic Attraction is the attraction between __________ charged particles.

• same 
• oppositely
• two positively
• two negatively

Multiple Choice

As the distance between protons and electrons increases, the force of attraction

• remains the same
• increases
• decreases
• is not affected

Multiple Choice

If distance remains the same, as the number of protons increases, the force of attraction

• remains the same
• increases
• decreases
• is divided by 1/2

Multiple Choice

What are the two variables that affect Coulombic Attraction?

• Distance and number of protons

• Number of neutrons and number of protons

• Number of neutrons

  and number of electrons

• Distance and number of electrons

Multiple Choice

Select the element that has the strongest Coulombic attraction.

• O

• S

• Se

• Te

Multiple Choice

Select the element that has the strongest Coulombic attraction.

• O

• F

• N

• C

Multiple Choice

Select the element that has the weakest Coulombic attraction.

• Fe

• Zn

• Mn

• Sc

Ionization Energy

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Multiple Choice

Using the interactive periodic table on the previous slide, what is the trend in ionization energy as you move ACROSS a period on the period table?

• Ionization energy INCREASES as you move across

• Ionization energy DECREASES as you move across

Multiple Choice

Using the interactive periodic table on the previous slide, what is the trend in ionization energy as you move DOWN a group on the period table?

• Ionization energy INCREASES as you move DOWN a group.

• Ionization energy DECREASES as you move DOWN a group.

IONIZATION ENERGY

Ionization energy: the amount of energy required to REMOVE an electron from an atom.

Trend across a period: Ionization energy INCREASES as you move across a period due to INCREASED Coulombic ATTRACTION. Since electrons are more attracted to the nucleus, they are harder to remove/pull away from the nucleus.

IONIZATION ENERGY

Ionization energy: the amount of energy required to REMOVE an electron from an atom.

Trend across a Group: Ionization energy DECREASES as you move DOWN a group due to DECREASING Coulombic ATTRACTION. Since electrons are less attracted to the nucleus, they are harder to remove/pull away from the nucleus.

Multiple Choice

What is ionization energy?

• Energy needed to destroy an atom
• Energy required to remove an electron
• Energy needed to split an electron
• Energy required to add an electron

Multiple Choice

Which element has the greater ionization energy?

• Magnesium (Mg)

• Phosphorus (P)

Multiple Choice

Which element has the greater ionization energy?

• Iodine (I)

• Chlorine (Cl)

ELECTRONEGATIVITY

ELECTRONEGATIVITY

Electronegativity: Electronegativity is an atom's ability to attract shared electrons in a bond.

Trend across a period: Electronegativity INCREASES as you move ACROSS a period of the periodic table. This is due to INCREASED Coulombic attraction. As electrons are more attracted to an atom's nucleus, it is easier to attract electrons in a bond.

ELECTRONEGATIVITY

Electronegativity: Electronegativity is an atom's ability to attract shared electrons in a bond.

Trend across a period: Electronegativity DECREASES as you move DOWN a period of the periodic table. This is due to DECREASED Coulombic attraction. As electrons are more attracted to an atom's nucleus, it is easier to attract electrons in a bond.

Multiple Choice

What does electronegativity do as you go across a period?

• decrease

• no pattern

• stay the same

• increase

Fill in the Blank

Electronegativity _________ as you go down a group.

Multiple Choice

Why does electronegativity decrease as you go down a group?

• As you go down a group, the outer electrons are further away from the nucleus

• As you go down a group, the nucleus is less able to attract electrons in a bond

• Both of these

• None of these

Multiple Choice

The element with the largest electronegativity in the halogens is - 

• At
• F
• Cl
• Br

Multiple Choice

The element with the lowest electronegativity in Period 3 is -

• Na

• Cl

• Ar

• Mg

Multiple Choice

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

• decreases, increases 
• increases, increases
• increases, decreases 
• stays the same, increases

ATOMIC RADIUS

ATOMIC RADIUS

Atomic Radius: Atomic radius is the distance from the nucleus to the outermost electron.

Trend across a period: Atomic radius DECREASES as you move across a period because of INCREASED Coulombic Attraction. As the attraction increases, electrons are pulled more tightly to the nucleus resulting in a SMALLER radius.

ATOMIC RADIUS

Atomic Radius: Atomic radius is the distance from the nucleus to the outermost electron.

Trend down a group: Atomic radius INCREASES as you move down a group because of DECREASED Coulombic Attraction. As the attraction decreases, electrons are allowed to spread out more from the nucleus resulting in a LARGER radius.

Multiple Choice

As you move down a group, atomic radius increases because - 

• you add more and more neutrons
• you add more and more protons
• you add more and more shells (energy levels)
• you add more atomic mass

Multiple Choice

As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 

• the number of protons increases, so attraction to electrons increases
• the number of energy levels increases
• the number of electrons increases
• the atomic mass increases

Multiple Choice

Which of the following will have a larger radius than Zinc?

• Gallium
• Aluminum
• Magnesium
• Strontium

Multiple Choice

Which periodic group has the smallest atomic radius?

• Alkali metals
• Halogens
• Noble Gases
• Transition metals

Multiple Choice

The atom with the largest atomic radius in Group 18 is - 

• Ar
• He
• Kr
• Rn

Multiple Choice

Atomic radius generally increases as we move __________.  

• down a group and from right to left across a period 
• up a group and from left to right across a period 
• down a group and from left to right across a period 
• up a group and from right to left across a period 

Multiple Choice

Which element's atom is larger? Nitrogen or Phosphorus?

• Nitrogen

• Phosphorus

Multiple Choice

Which atom has the largest atomic radius?

• potassium
• rubidium 
• francium
• cesium

Reorder

Put in order from biggest to smallest (decreasing size)

• Calcium

• Iron

• Zinc

• Bromine

• Krypton

1

2

3

4

5

• 1
• 2
• 3
• 4
• 5

If you want - Label on your periodic table

Note: you don't have to draw the arrows as large as they are on this, but it would be handy to have these labeled as we practice with this.

If you want - Label on your periodic table

Note: you don't have to draw the arrows as large as they are on this, but it would be handy to have these labeled as we practice with this.

If you want - Label on your periodic table

Note: you don't have to draw the arrows as large as they are on this, but it would be handy to have these labeled as we practice with this.

Mixed Practice

Multiple Choice

Which atom has the most valence electrons

• Ca

• C

• Cl

• Si

Multiple Choice

As you move across the periodic table, from left to right, ionization energy is __________________.

• decreasing

• increasing

Multiple Choice

Which atom is more electronegative?

• K

• Rb

• Cl

• B

Multiple Choice

As you move down the periodic table, atoms tend to get bigger because...

• They have more mass

• They have more protons

• They have more energy levels

• They have more mass

Multiple Choice

Which statement correctly and completely identifies a trend?

• Atomic radius decreases across a period, and increases down a group

• Electronegativity decreases across a period and decreases down a group

• Ionization energy increases across a period and increases down a group

Multiple Choice

Which atom has the largest radius

• Mg

• B

• S

• Br

Multiple Choice

Put the following in order of increasing ionization energy:Strontium, Aluminum, Indium

• Strontium, Indium, Aluminum
• Strontium, Aluminum, Indium
• Indium, Aluminum, Strontium
• Aluminum, Indium, Strontium

Multiple Choice

Put the following in order of increasing ionization energy:Cobalt, Tungsten, Ruthenium

• Tungsten, Ruthenium, Cobalt
• Cobalt, Tungsten, Ruthenium
• Ruthenium, Cobalt, Tungsten
• Cobalt, Ruthenium, Tungsten

Multiple Choice

Put these in increasing order of atomic radii:
F, N, B

• B < N < F
• B < F < N
• N < F < B
• F < N < B

Multiple Choice

The element with the lowest electronegativity in Period 3 is - 

• Na
• Cl
• Ar
• Mg