FREE CHEMISTRY AND STUDY GAMES ABOUT PERIODIC

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FREE CHEMISTRY AND STUDY GAMES ABOUT PERIODIC

TRENDS EXAM QUESTIONS

Actual Qs and Ans Expert-Verified Explanation

This Exam contains:

-Guarantee passing score -14 Questions and Answers -format set of multiple-choice -Expert-Verified Explanation Question 1: Trends in Ionization energy going left to right across a period: 2 reasons

Answer:

Ionization Energy INCREASE going across a period 1: Increasing nuclear charge means the nucleus has a better hold on the outer electrons.2: Decreasing atomic radius means that the outermost shell is closer to the nucleus and is therefore held tighter.

Question 2: Reactivity of the Alkali Metals

Answer:

Increases as we go down the group.All the elements have only 1 electron on their outer shell.Losing this electron gives them a full outer shell.This means they have a low ionisation energy and electronegativity.

Question 3: Electronegativity

Answer:

A measure of an atom's ability to attract and hold electrons in a molecule. Will predict how atoms combine chemically. Linus Pauling developed the electronegativity scale.

Question 4: Ionization Energy

Answer:

The first ionization energy of at atom is the minimum energy required to completely remove the most loosely bound electron from a neutral atom in a gaseous state. Noble Gases have the highest Ionization Energy levels, as they have full outer energy level

Question 5: Trends in Electronegativity going down a group. 2 reasons

Answer:

Electronegativity DECREASES as we go down a group 1: Increasing atomic radius means the electrons are further away from the attractive force of the nucleus.2: The screening effect of the inner negative electrons block the pull of the positive nucleus.Question 6: Trends in Electronegativity going left to right across a period. 2 reasons

Answer:

Electronegativity INCREASES going across a period.1: Increasing nuclear charge means the nucleus has a stronger hold on the electrons.2: Decreasing atomic radius: as no new shell is being added the stronger nucleus can hold the outer electrons tighter

Question 7: Properties of Alkali Metals

Answer:

1: Easier to cut as we move down the group.

2: Display more vigorous reaction with water as we move down the group.

3: Tarnish with air faster as we move down the group.

Question 8: Trends in Atomic Radius going down a group. 2 reasons

Answer:

Atomic radius INCREASES.

1: A new shell is being added as we move down the table.

2: The screening effect of the extra electrons cancels out the pull of the growing nucleus.

Question 9: Trends in Electron Affinity going left to right across a period

Answer:

INCREASES from left to right along a period

• as energy level continues to fill it has a stronger attraction for the elecrons.

Question 10: Electron Affinity

Answer:

The amount of energy required to add an electron to a neutral atom to form a negative ion or anion.How strongly an atom attracts additional electrons

Question 11: Reactivity of the Halogens

Answer:

Reactivity increases moving up the group.

1: Decreasing atomic radius brings the outer shell closer to the nucleus.

2: Electronegativity increases as we move up the group.

3: All the halogens require only 1 electron to achieve noble gas structure

Question 12: Trends in Atomic Radius going left to right across a period. 2 reasons

Answer:

Atomic radius DECREASES

1: Increasing nuclear charge due to an extra proton being added

2: There is no increase in screening effect as no new shell is being added

Question 13: Trends in Ionization energy going down a group: 2 reasons

Answer:

Ionization Energy DECREASES going down a group.

1: As atomic radius increases the electrons are further away from the nucleus.

2: The screening effect of the inner electrons cancels out the pull of the nucleus.

Question 14: Atomic Radius

Answer:

Atomic radius is defined as half the distance between the nuclei of atoms of the same element that are joined by a single covalent bond.