Periodic Trends

Which elements in Group 16 has the greatest tendency to gain electrons? A.)Se B.)S C.)O D.)Te

D.)Te

Compared the Atomic Radius of a sodium atom, the atomic radius of a magnesium atom. The smaller radius is primarily the result of the magnesium atom having... A.)A larger nuclear charge B.)more principal energy levels C.)Smaller nuclear charge D.)fewer principals energy levels,

A.) A larger nuclear charge

The Group 17 element with the highest electronegativity is... A.)Fluorine B.)Iodine C.)Bromine D.)Chlorine

A.) Fluorine

Which element in Period 5 of the Periodic Table is a transition element? A.)Ag B.)Sb C.)Xe D.)Sr

A.)Ag

Which element is a member of the halogen family? A.)I B.)B C.)S D.)K

A.)I

Which group 17 element has the least attraction for electrons? A.)I B.)F C.)Cl D.)Br

A.)I

As each successive elements in Group 15 of the Periodic Table is considered in order of increasing atomic number, the atomic radius... A.)Increases B.)Remains the Same C.)Decreases

A.)Increases

Which electron configuration represents a transition element? A.)[Ar] 3d^5 4s^2 B.)[Ar] 3d^10 4s^2 4p^6 C.)1s^2 2s^2 2p^5 D.)[Ne] 3s^2

A.)[Ar] 3d^5 4s^2

Which atom in these pairs has the largest atomic radius? Al or B

Al

Which atom has the lowest ionization energy? Aluminum, Silicon, Phosphorus, or Sulfur?

Aluminum

Which atom in these pairs has the greater ionization energy? P or Ar

Ar

Which is smaller? Nitrogen's atom or ion?

Atom

Which would be the larger? Calcium: The Ionic radius or the Atomic radius?

Atomic radius

Which would be the larger? Potassium: The Ionic radius or the Atomic radius?

Atomic radius

As elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to... A.)Decreasing Radius and increasing Shielding Effect B.)Increasing Radius and increasing Shielding Effect C.)Increasing Radius and decreasing Shielding Effect. D.)Decreasing Radius and decreasing .

B.) Increasing Radius and increasing Shielding Effect.

Which statement best describes Group 2 element as they are considered in order from top to bottom of the Periodic table? A.) The number of principal energy levels increases, and the number of valence electrons increases. B.) The number of principal energy levels increases, and the number of valence electrons remains the same. C.)The number of principal energy levels remains the same, and the number of valence electrons increases. D.)The number of principal energy levels remains the same, and the number of valence electrons decreases.

B.) The number of principal energy levels increases, and the number of valence electrons remains the same.

The amount of energy required to move the outermost electron from a gaseous atom in the ground state is known as... A.)Electronegativity B.)First Ionization Energy C.)Activation Energy D.)Conductivity

B.)First Ionization Energy

The ability of carbon to attract electrons is... A.)Less than that of nitrogen, but greater than that of oxygen. B.)Less than that of nitrogen and oxygen C.)Greater than that of nitrogen, but lesser than that of oxygen. D.)Greater than that of nitrogen and oxygen.

B.)Less than that of nitrogen and oxygen.

Which of these elements has the least attraction for electrons in a chemical bond? A.)Chlorine B.)Nitrogen C.)Fluorine D.)Oxygen

B.)Nitrogen

On the periodic table of the elements, all the elements within Group 16 have the same... A.)Protons B.)Valence Electrons C.)Neutrons D.)Energy Levels

B.)Valence Electrons

Which atom in these pairs has the greater ionization energy? Li or Be

Be

Which atom has the largest electronegativity? Calcium, Beryllium, Radium, or Magnesium?

Beryllium

Which atom has the highest electronegativity? Boron, Indium, Aluminum, or Gallium?

Boron

Which atom in these pairs has the greater electronegativity? Br or As

Br

Which atom in these pairs has the largest atomic radius? Br or Cl

Br

Which atom has the largest ionization energy? Calcium, Bromine, Arsenic, or Iron?

Bromine

What is the total number of valence electrons in an atom of xenon, Xe? A.)2 B.)18 C.)8 D.)0

C.)8

Which list of elements from group 2 on the Periodic Table is arranged in order of increasing Atomic Radius? A.)Ca, Mg, Be B.)Cl, Br, I C.)Al, Si, P D.)N, C, B

C.)Al, Si, P

As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element generally... A.)Increases B.)Remains the Same C.)Decreases

C.)Decreases

Which noble gas has the highest first ionization energy? A.)Neon B.)Krypton C.)Helium D.)Radon

C.)Helium

As the elements Li to F in Period 2 of the Periodic Table are considered in succession, how do the relative electronegativity and the covalent radius of each successive element compare? A.)The relative electronegativity decreases, and the atomic radius decreases. B.)The relative electronegativity decreases, and the atomic radius increases. C.)The relative electronegativity increases, and the atomic radius decreases. D.)The relative electronegativity increases, and the atomic radius increases.

C.)The relative electronegativity increases, and the atomic radius decreases.

Which atom in these pairs has the greater ionization energy? Ca or Ba

Ca

Which atom in these pairs has the largest atomic radius? Mg or Ca

Ca

Which atom has the biggest atomic radius? Krypton, Zinc, Calcium, or Bromine?

Calcium

Which has the lower ionization energy? Beryllium or Calcium?

Calcium

Which atom has the lowest ionization energy? Nitrogen, Fluorine, Oxygen, or Carbon?

Carbon

Which has the larger atomic nucleus? Carbon or Fluorine?

Carbon

Which atom has the highest electronegativity? Chlorine, Sulfur, Aluminum, or Magnesium?

Chlorine

Which atom has the largest size? Chlorine, Sodium, Silicon, or Aluminum?

Chlorine

Which atom in these pairs has the greater electronegativity? Cl or S

Cl

Which atom in these pairs has the greater ionization energy? Cl or Si

Cl

Determine the element from the excited state electron configuration and write the ground state electron configuration. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^8 5p^1

Copper

An element with a partially filled d sublevel in the ground state is classified as... A.)An Alkaline Earth Metal B.)A Halogen C.)An Alkali Metal D.)A Transition Metal

D.) A Transition Metal

The strength of an atom's attraction for the electrons in a chemical bond is the atom's... A.)Ionization Energy B.)Heat of reaction C.)Heat of Formation D.)Electronegativity

D.) Electronegativity

Which properties are most common in nonmetals? A.)Low Ionization Energy and Low Electronegativity. B.)High Ionization Energy and Low Electronegativity. C.)Low Ionization Energy and High Electronegativity. D.)High Ionization Energy and High Electronegativity.

D.) High Ionization Energy and High Electronegativity.

What is the total number of valence electrons in an atom of boron in the ground state? A.)5 B.)7 C.)1 D.)3

D.)3

Which sequences of elements is arranged in order of decreasing atomic radii? A.)Cl, Br, I B.)Li, Na, K C.)N, C, B D.)Al, Si, P

D.)Al, Si, P

Which of the following Group 2 elements has to take the lowest first ionization energy? A.)Mg B.)Ca C.)Be D.)Ba

D.)Ba

The elements calcium and strontium have similar chemical properties because they both have the same... A.)Number of completely filled sublevels B.)Mass number C.)Atomic number D.)Number of valence electrons

D.)Number of valence electrons

Indicate whether the following properties increase or decrease from left to right across that periodic table. Atomic Radius (excluding noble gases)

Decrease

Atomic Radius ____ across a period and ____ down a group.

Decrease, increase

Why does fluorine have a higher ionization energy than iodine?

Energy is required to move an electron, and ionization decreases as you go down a group.

Which atom has the lowest ionization energy? Iodine, Bromine, Fluorine, or Chlorine?

Iodine

Which atom in these pairs has the greater electronegativity? Ca or Ga

Ga

Indicate whether the following properties increase or decrease from left to right across that periodic table. Electronegativity

Increase

Indicate whether the following properties increase or decrease from left to right across that periodic table. First Ionization Energy

Increase

Electronegativity ____ across a period and ____ down a group.

Increase, decrease

Ionization Energy ____ across a period and ____ down a group.

Increase, decrease

Which is smaller? Magnesium's atom or ion?

Ion

Which would be the larger? Bromine: The Ionic radius or the Atomic radius?

Ionic radius

Which would be the larger? Fluorine: The Ionic radius or the Atomic radius?

Ionic radius

Which atom in these pairs has the greater ionization energy? Li or K

Li

Which atom has the biggest atomic radius? Lithium, Carbon, Nitrogen, or Fluorine?

Lithium

Which atom has the highest electronegativity? Nitrogen, Calcium, Francium, or Silicon?

Lithium

Which atom has the lowest ionization energy? Lithium, Beryllium, Boron, or Carbon?

Lithium

Which atom in these pairs has the greater ionization energy? Na or Ba

Na

Which atom in these pairs has the largest atomic radius? Na or Al

Na

Rank the following elements by increasing electronegativity: Sulfur, oxygen, neon, Aluminum.

Neon, aluminum, sulfur, oxygen.

Which atom in these pairs has the greater electronegativity? Li or O

O

Which atom in these pairs has the greater electronegativity? O or S

O

Which atom in these pairs has the largest atomic radius? O or F

O

Rank the following elements by increasing atomic radius: Carbon, aluminum, oxygen, potassium.

Oxygen, Carbon, Aluminum, oxygen, potassium.

Which atom has the biggest atomic radius? Polonium, Sulfur, Oxygen, or Tellurium?

Polonium

Which atom has the biggest atomic radius? Calcium, Beryllium, Radium, or Magnesium?

Radium

Determine the element from the excited state electron configuration and write the ground state electron configuration. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5p^1

Rubidium

Which atom in these pairs has the largest atomic radius? S or O

S

Which atom in these pairs has the greater electronegativity? Ba or Sr

Sr

What trend in atomic radius occurs down a group on the periodic table? What causes this trend?

The energy increases because energy required is greater.

Define electronegativity.

The tendency for an atom to attract electrons to itself when it is chemically combined with another element.

Why do elements in the same family generally have similar properties?

They have similar atomic valence.