Electron Shielding

Multiple Choice

The concept of shielding happens because of

• attraction between nucleus and valence electrons

• attraction between nucleus and core electrons

• repulsion between valence electrons and other valence electrons

• repulsion between core electrons and valence electrons

Multiple Choice

How many shielding electrons are in this atom: 1s² 2s²2p⁶

• 2

• 4

• 6

• 8

Multiple Choice

How many shielding electrons are in: 1s²2s²2p⁶3s²3p⁶4s²

• 2

• 4

• 10

• 18

Multiple Choice

Shielding electrons are

• in the highest energy level

• in the lower energy levels

Multiple Choice

Valence electrons are

• in the highest energy orbitals

• closest to the nucleus

Multiple Choice

The effective nuclear charge is _ the actual nuclear charge

• the same as

• less than

• greater than

Multiple Choice

When a new energy level is added to the atom, shielding

• increases

• decreases

Multiple Choice

Which will definitely have a larger radius than zinc?

• Gallium

• Aluminum

• Magnesium

• Strontium

Multiple Choice

When you move across the periodic table, atomic radius _. When you move down the table, atomic radius _.

• increases, decreases

• decreases, increases

• increases, increases

• decreases, decreases

Multiple Choice

Which atom has the largest atomic radius?

• potassium

• rubidium 

• francium

• cesium

Multiple Choice

As you move down the periodic table, atoms get bigger.  This is because _.

• The atoms have more mass.

• The atoms have more protons.

• The atoms have more energy levels

• The atoms have more nuetrons

Multiple Choice

As you move down the periodic table atoms get bigger.  This is because _.

• The atoms have more mass.

• The atoms have more protons.

• The atoms have more energy levels

• The atoms have more nuetrons

Multiple Choice

As you move across the periodic table, atoms tend to get smaller because, _.

• the atoms have more mass, which increases the gravitational pull

• it doesn't, atoms get bigger going from left to right because of the additional protons and electrons that are being added.

• effective nuclear charge tends to increase

• atoms lose energy levels make them smaller

Multiple Choice

Which is larger

• P

• P^3-

Multiple Choice

Which is larger

• Na

• Na⁺

Multiple Choice

Which is larger

• S

• S^2-

Multiple Choice

Which is ions is larger

• Ca²⁺

• Mg²⁺

Multiple Choice

Ionization energy is

• the energy required to add an electron to a specific atom

• how much energy it takes to remove an electron from an atom

• the energy required to shield the outer electrons from the nucleus

• a measure of the ability of an atom to attract electrons

Multiple Choice

Which of the following is true for alkaline earth metals as their atomic number increases?

• The atomic radius decreases.

• Ionization energy decreases.

• The number of valence electrons increases.

• The Coulomb attraction increases.

Multiple Choice

Which corresponds to a correct trend in ionization energy?

• Cl > S > P > Al

• Sr > Ca > Mg > Be

• Rb > K > Na > Li

• Rb > Sr > I > Xe

Multiple Choice

Which is true about a sulfur atom and a chlorine atom?

• Sulfur is larger and has higher ionization energy.

• Sulfur is larger and has lower ionization energy.

• Sulfur is smaller and has higher ionization energy.

• Sulfur is smaller and has lower ionization energy.

Multiple Choice

The graph shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?

• E drops significantly moving down a group because valence electrons are in higher n

• E increases gradually across a period because valence electrons are in higher n

• E increases gradually across a period because Z increases

• E increases when valence electrons are more attracted to the nucleus

Labelling

Where can we find the following atoms?

Drag labels to their correct position on the image

oxygen

aluminum

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

Electronegativity is

• how much an atom wants electrons in a bond

• the ability of an atom to lose electrons

• the energy required to remove an electron from a specific atom

• how easy it is to make friends.

Multiple Choice

As you move down a group, there are _ electrons and energy levels leading to a greater shielding effect and a _ electronegativity value.

• more, higher

• more, lower

• less, higher

• less, lower

Multiple Choice

Which correctly places the halogens in order of increasing electronegativity?

• F, Cl, Br, I

• Cl, F, Br, I

• I, Br, Cl, F

• Br, Cl, I, F

Multiple Choice

Put the following in order of increasing ionization energy

• Lithium, Carbon, Neon

• Carbon, Lithium, Neon

• Neon, Carbon, Lithium

• Lithium, Neon, Carbon