Chemistry Chapter 5 Review

Questions and Answers

Mendeleev organized the elements by their ____________?

properties

What do you call the rows going across the periodic table?

periods

What does the periodic law state?

the physical and chemical properties of the elements are functions of their atomic number.

A carbon atom in its ground state has how many electrons in its outermost shell?

4 Signup and view all the answers

Based on the periodic law, what element is most similar in behavior to Sulfur (S)?

Chlorine (Cl) Signup and view all the answers

The electron configuration of main-group elements ends in ________________?

s & p orbitals Signup and view all the answers

How many periods of elements are in the periodic table?

7 Signup and view all the answers

The discovery of noble gases changed Mendeleev's version of the periodic table by adding a new ______________?

group Signup and view all the answers

In a group of elements, as the atomic number increases the atomic radius _________________________?

generally increases Signup and view all the answers

As electrons are removed one by one from an atom, what happens to the ionization energy for the next electron to be removed?

it increases Signup and view all the answers

What group are the alkali metals found in?

Group 1 Signup and view all the answers

An important attribute of noble gases is that they are _______________?

largely unreactive Signup and view all the answers

How many valence electrons are in Group 2?

2 Signup and view all the answers

How do valence electrons differ from regular electrons?

Valence electrons are the outer electrons that can leave the atom to take part in chemical reactions. Signup and view all the answers

If an element has the electron configuration [Kr]4d^10/5s^2/5p^5, it is located in which period?

5th period Signup and view all the answers

The measure of the ability of an atom in a chemical compound to attract electrons is called _________________

electronegativity Signup and view all the answers

An atom or group of atoms that has a + or - charge is called an ___________?

ion Signup and view all the answers

If an element had the electron configuration [Xe]4f^14/5d^10/6s^2, what period, group, and block is it in?

Period 6, Group 12, d block Signup and view all the answers

What are the elements in Group 2 called?

alkaline-earth metals Signup and view all the answers

The energy required to remove an electron from an atom is called its ___________________________?

ionization energy Signup and view all the answers

1/2 the distance between the nuclei of identical atoms that are bonded together is the ______________________?

atomic radius Signup and view all the answers

The atomic number tells you the number of ____________?

protons Signup and view all the answers

Elements at the right end of the p-block are ___________________________ compared to elements at the left end.

less metallic Signup and view all the answers

What group are the halogens located in?

Group 17 Signup and view all the answers

What are the elements called that are 58-71 on the periodic table?

Lanthanides Signup and view all the answers

What are the elements called that are 90-103 on the periodic table?

Actinides Signup and view all the answers

What general trend(s) does atomic radius follow?

It decreases as you move right in a period. It increases as you move down a group. Signup and view all the answers

What elements have the highest ionization energy?

the noble gases (Group 18) Signup and view all the answers

When you move up a group on the periodic table, why does the ionization energy increase?

the valence electrons are closer to the nucleus Signup and view all the answers

Arrange the following elements in order of decreasing ionization energy: Gallium (Ga), Krypton (Kr), Calcium (Ca), and Arsenic (As)

Kr, As, Ca, Ga Signup and view all the answers

Why does the atomic radius decrease as you move down a group?

The number of energy levels increases as you move down a group. Each subsequent energy level is further from the nucleus than the last. Signup and view all the answers

From to ___________ electronegativity increases.

left to right Signup and view all the answers

What alkali metal has the highest ionization energy?

Lithium (Li) Signup and view all the answers

Name the element in Period 3 with the smallest atomic radius?

Argon (Ar) Signup and view all the answers

What element in Group 14 has the largest electronegativity?

Carbon (C) Signup and view all the answers

What section (Groups) of elements are the transition metals in?

Group 3-12 Signup and view all the answers

How many valence electrons does Sulfur have?

6 Signup and view all the answers

Study Notes

Periodic Table Organization

Mendeleev organized elements based on their properties.
Rows across the periodic table are called periods.
The periodic law indicates that properties of elements relate to their atomic number.

Atomic Structure and Behavior

A ground state carbon atom has 4 electrons in its outermost shell.
Sulfur (S) is most similar to Chlorine (Cl) in behavior, according to periodic law.
Main-group elements have electron configurations ending in s & p orbitals.

Periods and Groups

There are 7 periods of elements in the periodic table.
Noble gases added a new group to Mendeleev's periodic table.
Alkali metals are located in Group 1, while alkaline-earth metals are in Group 2.

Atomic Characteristics

As atomic number increases in a group, the atomic radius generally increases.
Ionization energy increases as electrons are sequentially removed from an atom.
Valence electrons differ from regular electrons as they participate in chemical reactions.

Electron Configuration

An element with the configuration [Kr]4d^10/5s^2/5p^5 is in the 5th period.
An element with the configuration [Xe]4f^14/5d^10/6s^2 is in the 6th period, Group 12, and d block.

Electronegativity and Ions

Electronegativity measures an atom's ability to attract electrons in a compound.
An ion is defined as an atom or group of atoms with a positive or negative charge.

Atomic Radius and Trends

Atomic radius is half the distance between nuclei of identical bonded atoms.
The atomic number represents the number of protons in an element.
Elements on the right end of the p-block are less metallic than those on the left.

Groups of Elements

Halogens are found in Group 17.
Elements numbered 58-71 on the periodic table are known as Lanthanides.
Elements numbered 90-103 are known as Actinides.

Trends in Atomic Characteristics

Atomic radius decreases across a period and increases down a group.
Noble gases (Group 18) exhibit the highest ionization energy.
Ionization energy increases moving up a group due to proximity of valence electrons to the nucleus.

Ionization Energy Order

The order of decreasing ionization energy among Gallium (Ga), Krypton (Kr), Calcium (Ca), and Arsenic (As) is: Kr, As, Ca, Ga.

Atomic Radius Variations

The atomic radius increases down a group because additional energy levels are added, distancing electrons from the nucleus.

Electronegativity Trends

Electronegativity increases as one moves from left to right across a period.
Lithium (Li) has the highest ionization energy among alkali metals.

Specific Element Characteristics

Argon (Ar) in Period 3 has the smallest atomic radius.
Carbon (C) has the largest electronegativity in Group 14.
Transition metals are located in Groups 3-12.

Valence Electrons

Sulfur has 6 valence electrons, essential for determining its chemical reactivity.

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Test your knowledge of key concepts in Chemistry Chapter 5 with these flashcards. Covering topics like the periodic table, Mendeleev's organization of elements, and the periodic law, this quiz will help reinforce your understanding of essential chemistry principles.