Chemical Periodicity

Which atom in each pair has the largest atomic radius? 1. Al or B 2. Na or Al 3. S or O 4. O or F 5. Br or Cl 6. Mg or Ca

1. Al 2. Na 3. S 4. O 5. Br 6. Ca

Which atom in each pair has the greater Ionization Energy? 1. Li or Be 2. Ca or Ba 3. Na or K 4. P or Ar 5. Cl or Si 6. Li or K

1. Be 2. Ca 3. Na 4. Ar 5. Cl 6. Li

Which atom in each pair has the greater Electronegativity? 1. Ca or Ga 2. Br or As 3. Li or O 4. Ba or Sr 5. Cl or S 6. O or S

1. Ga 2. Br 3. O 4. Sr 5. Cl 6. O

Define Shielding.

A barrier made of inner-shell electrons that serves to decrease the pull of the nucleus on the outer electrons.

Compared to the atomic radius of a sodium atom, the atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having: A. A larger nuclear charger B. A smaller nuclear charge C. More principal energy levels D. Fewer principal energy levels

A. A larger nuclear charge

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

A. Al, Si, P

Which list of elements from group 2 on the periodic table is arranged in order of increasing atomic radius? A. Be, Mg, Ca B. Ca, Mg, Be C. Ba, Ra, Sr D. Sr, Ra, Br

A. Be, Mg, Ca

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. Decreases B. Increases C. Remains the same

A. Decreases

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

A. Electronegativity

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

A. First Ionization Energy

The group 17 element with the highest Electronegativity is: A. Fluorine B. Chlorine C. Bromine D. Iodine

A. Fluorine

On the periodic table of elements, all the elements within group 16 have the same number of: A. Valence electrons B. Energy levels C. Protons D. Neutrons

A. Valence electrons

Indicate whether the following properties increase or decrease from left to right across the periodic table: Atomic Radius(excluding noble gases), First Ionization Energy, Electronegativity.

Atomic Radius (excluding noble gases): Decreases. First Ionization Energy: Increases. Electronegativity: Increases.

What trend in Atomic Radius occurs down a group on the periodic table? What causes this trend?

Atomic Radius increases down a group because energy levels (shells) are added.

An element with a partially filled d sublevel in the ground state is classified as: A. A halogen B. A transition metal C. An alkali metal D. An alkaline earth metal

B. A transition metal

Which sequence correctly places the elements in order of increasing Ionization Energy? A. H > Li > Na > K B. I > Br > Cl > F C. O > S > Se > Te D. H > Be > Al > Ga

B. I > Br > Cl > F

As each successive element in group 15 of the periodic table is considered in order of increasing atomic number, the atomic radius: A. Decreases B. Increases C. Remains the same

B. Increases

Which of the following atoms has the largest atomic radius? A. Na B. K C. Mg D. Ca

B. K

Which statement best describes Group 2 elements 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 stay 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 stays the same.

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

C. 3

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

C. 8

Which element in period 5 of the periodic table is a transition element? A. Sr B. Sb C. Ag D. Xe

C. Ag

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

C. I

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

C. Nitrogen

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

C. Number of valence electrons

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

C. [Ar]3d^5 4s^2

Which of the following group 2 elements has the lowest First Ionization Energy? A. Be B. Mg C. Ca D. Ba

D. Ba

Which noble gas has the highest first Ionization Energy? A. Radon B. Krypton C. Neon D. Helium

D. Helium

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

D. High Ionization Energy and high Electronegativity

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

D. I

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 decreasing shielding effect B. Decreasing radius and increasing shielding effect C. Increasing radius and decreasing shielding effect D. Increasing radius and increasing shielding effect

D. Increasing radius and increasing shielding effect

The ability of Carbon to attract electrons is: A. Greater than that of Nitrogen, but less than that of Oxygen B. Less than that of Nitrogen, but greater than that of Oxygen C. Greater than that of Nitrogen and Oxygen D. Less than that of Nitrogen and Oxygen

D. Less than that of Nitrogen and Oxygen

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

D. O

Define Ion Size.

Different number of electrons.

Why does Fluorine have a higher ionization energy than Iodine?

Fluorine has a smaller atomic radius, so the protons can exert a greater pull on electrons.

Define Reactivity.

How easily a metal atom loses its electrons (low ionization energy) determines the reactivity of the metals and how easily a non-metal atom gains electrons (high electron affinity) determines the reactivity of the non-metals.

What trend in Ionization Energy occurs across a period on the periodic table? What causes this trend?

Ionization Energy increases across a period because as elements become less metallic, it requires more energy to remove an electron.

Rank the following elements by increasing electronegativity: Sulfer, Oxygen, Neon, Aluminum.

Neon, Aluminum, Sulfer, Oxygen.

Rank the following elements by increasing atomic radius: Carbon, Aluminum, Oxygen, Potassium.

Oxygen, Carbon, Aluminum, Potassium.

Define Multiple Ionization Energies.

Removal of a second, third, fourth, and subsequent electrons from an atom. As more electrons are removed from an atom, we notice that there are places where there seems to be a big JUMP in the energy required to remove an electron.

Define Ionization Energy.

The amount of energy required to remove the most loosely-held electron (ONE electron) from an atom or an ion (usually the outermost electron); it is sometimes called ionization potential.

Define Electron Affinity.

The amount of energy that is absorbed or given off when an atom is forced to accept an electron. Affinity is defined as "a natural attraction" so ELECTRON AFFINITY is a natural attraction for electrons.

Define Atomic Radius.

The size of atom; distance from the nucleus to the outer edge of the atom; one-half the diameter of the atom - the atomic radius cannot be measured exactly because an atom does not have a sharply -defined boundary.

Define Electronegativity.

The tendency of an atom to pull electrons that are bonded closer to itself and, perhaps, add them to its outer energy level.

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

They have the same Valence Shell electron arrangement.