Unit 4 (H) Review

1

Which of the following has the largest atomic radius?

Ca

Cl-

Sr

Ca+2

1

Why is Nitrogen smaller than its ion N^3- ?

It has less electrons than it's ion which means a stronger Z_eff .

It has more electrons than it's ion which means a stronger Z_eff .

It has less electrons than it's ion which means more shielding.

It has more electrons than it's ion which means more shielding.

1

Removing an additional electron requires

more energy than the one before it.

less energy than the one before it..

1

Which statement is FALSE?

Lithium is more reactive than Beryllium.

Neon is less reactive than Fluorine.

Potassium is more reactive than Lithium.

Iodine is more reactive than Fluorine.

1

Which of the following statements is true?

Nitrogen has a higher ionization energy than Boron and a higher electronegativity.

Nitrogen has a higher ionization energy than Boron and a lower electronegativity.

Nitrogen has a lower ionization energy than Boron and a higher electronegativity.

Nitrogen has a lower ionization energy than Boron and a lower electronegativity.

1

Select all the true statements about the element Phosphorous.

Has 5 valence electrons.

Has on oxidation number of +3.

Will tend to gain electrons

Is less electronegative than argon.

Has a larger atomic radius than aluminum.

Has a stronger effective nuclear charge than aluminum.

Obavezno

1

The reason a color is emitted when a metal compound is burned is because the electron

moves to an excited state

is removed from the element

falls back to its ground state

Obavezno

1

1s²2s²2p⁶3s²3p⁶4s²3d³ is the electron configuration for

Obavezno

1

Which of the following elements will have similar chemical properties to oxygen?

Obavezno

1

X-ray diffraction was used on unknown Element Z to find there are about 159 pm (picometers) between the center of Element Z's nucleus and its outermost electrons. The same measurement was done on 5 other known elements and that data was recorded in the table below. Using the table, which element could fit Element Z's description above?

Obavezno

1

Why does ionization energy decrease down a group?

Shielding increases

Nuclear charge decreases

Shielding decreases

Valence electrons decrease

Obavezno

1

Which group in the periodic table has 7 valence electrons?

Transition Metals

Alkaline Earth Metals

Halogens

Alkali Metals

1

The ionization energy increases as you move across a period because

the effective nuclear charge increases as protons are added.

the effective nuclear charge decreases as protons are added.

shielding increases as shells are added.

shielding increases as electrons are added.

Unit 4 (H) Review

Which of the following has the largest atomic radius?

Why is Nitrogen smaller than its ion N3- ?

Removing an additional electron requires

Which statement is FALSE?

Which of the following statements is true?

Select all the true statements about the element Phosphorous.

The reason a color is emitted when a metal compound is burned is because the electron

1s22s22p63s23p64s23d3 is the electron configuration for

Which of the following elements will have similar chemical properties to oxygen?

Why does ionization energy decrease down a group?

Which group in the periodic table has 7 valence electrons?

The ionization energy increases as you move across a period because

Which of the following has the largest atomic radius?

Why is Nitrogen smaller than its ion N3- ?

Removing an additional electron requires

Which statement is FALSE?

Which of the following statements is true?

Select all the true statements about the element Phosphorous.

The reason a color is emitted when a metal compound is burned is because the electron

1s22s22p63s23p64s23d3 is the electron configuration for

Which of the following elements will have similar chemical properties to oxygen?

Why does ionization energy decrease down a group?

Which group in the periodic table has 7 valence electrons?

The ionization energy increases as you move across a period because

Why is Nitrogen smaller than its ion N^3- ?

1s²2s²2p⁶3s²3p⁶4s²3d³ is the electron configuration for

Why is Nitrogen smaller than its ion N^3- ?

1s²2s²2p⁶3s²3p⁶4s²3d³ is the electron configuration for