Chemistry Chapter 5 Quiz

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Which statement about the trends in density is true?

Density only increases in the first group of the periodic table.
Density reaches a peak at Aluminum (group 3, period 3). (correct)
Density is constant across a period.
Density decreases as you move down group 7.

The atomic size decreases as you move down a group in the periodic table.

False (B)

What is the covalent radius?

Half the distance between the nuclei of two bonded atoms.

Which element is known to have the highest melting point among those mentioned?

Carbon (A) Signup and view all the answers

Density measures mass per unit __________.

volume Signup and view all the answers

Melting and boiling points generally increase as you move down group 1 of the periodic table.

False (B) Signup and view all the answers

Match the following elements with their density trends:

Boron = Highest peak density in group 3, period 2 Aluminum = Peak density in group 3, period 3 He = Lowest density in group 0 Fr = Lowest density in group 1 Signup and view all the answers

Who invented the periodic table?

Dimitri Mendeleev Signup and view all the answers

The modern periodic table is based on _____ instead of atomic mass.

atomic number Signup and view all the answers

Match the following trends with their descriptions:

Melting points peak = Occurs at carbon for period 2 Boiling points peak = Occurs at silicon for period 3 Decreasing trend down a group = Melting and boiling points in group 1 Strength of attraction = Stronger on the left side of the table Signup and view all the answers

Who introduced the concept of electronegativity?

Linus Pauling (B) Signup and view all the answers

How does electronegativity change across a period?

It increases (C) Signup and view all the answers

Fluorine is the least electronegative element.

False (B) Signup and view all the answers

In the compound hydrogen iodide, which atom has a stronger attraction for the shared electrons?

Iodine Signup and view all the answers

Electronegativity increases as you move down a group in the periodic table.

False (B) Signup and view all the answers

In chlorine gas (Cl2), the electrons are shared __________.

equally Signup and view all the answers

What causes the decrease in electronegativity when moving down a group?

Shielding and increased distance from the nucleus. Signup and view all the answers

Electronegativity decreases going down a group due to increased __________.

shielding Signup and view all the answers

Match the elements with their electronegativity characteristic:

Fluorine = Most electronegative element Chlorine = Equal sharing of electrons Hydrogen = Slight positive charge in hydrogen iodide Iodine = Slight negative charge in hydrogen iodide Signup and view all the answers

Match the following factors with their effect on electronegativity:

Increased nuclear charge = Increases electronegativity Increased shielding = Decreases electronegativity Distance from nucleus = Decreases electronegativity Number of electron shells = Decreases electronegativity Signup and view all the answers

What is the first ionisation energy?

Amount of energy required to remove one mole of electrons from one mole of atoms in the gaseous state (A) Signup and view all the answers

Why does ionisation energy decrease down a group?

The outer electrons are further away from the nucleus due to increased electron shells. (C) Signup and view all the answers

Ionisation energy decreases across a period due to an increase in nuclear charge.

False (B) Signup and view all the answers

The first ionisation energy is always less than the second ionisation energy for any element.

True (A) Signup and view all the answers

What is the process that occurs during the second ionisation energy?

The removal of one mole of electrons from one mole of gaseous 1+ ions. Signup and view all the answers

What happens to the ionisation energy as successive electrons are removed from an atom?

It increases. Signup and view all the answers

The noble gas has the highest value for the __________ ionisation energy within each period.

first Signup and view all the answers

Match the following terms with their definitions:

First Ionisation Energy = Energy required to remove one mole of electrons from one mole of gaseous atoms Second Ionisation Energy = Energy required to remove one mole of electrons from one mole of gaseous 1+ ions Noble Gas = Element with full outer electron shell and highest ionisation energy within a period Ionisation Energy Trend Across Period = Increases due to greater nuclear charge Signup and view all the answers

The large jump in ionisation energy occurs when an electron is removed from a new ______.

shell Signup and view all the answers

Match the elements with their respective ionisation energy trends:

Potassium = Higher second ionisation energy due to stable electron configuration Magnesium = Lower second ionisation energy as it tends toward stable arrangement Lithium = Decreases in ionisation energy down the group Sodium = Experiences increased attraction on removal of electrons Signup and view all the answers

Periodic Trends in Melting/Boiling Points

Melting and boiling points of elements vary in a predictable pattern across the periodic table, influenced by intermolecular forces.

Peak Melting/Boiling Points

Elements like carbon (period 2) and silicon (period 3) have higher melting and boiling points than their neighbors.

Left-Right Melting/Boiling Point Trend

Attractive forces between particles tend to be stronger for elements on the left side of the periodic table.