Chemistry Chapter 3: Periodic Table Flashcards

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Questions and Answers

Who is known as the Father of the Periodic Table?

Thomson
Mendeleev (correct)
Curie
Mosley

Who developed the Modern Periodic Table?

Mosley (correct)
Rutherford
Mendeleev
Dalton

The Periodic Law states that elements are arranged by atomic mass.

False (B)

Define Groups in the periodic table.

Vertical columns where elements react similarly and have the same number of valence electrons. Signup and view all the answers

What is the name of Group 1 elements?

Alkali Signup and view all the answers

What is the name of Group 2 elements?

Alkaline Earth Signup and view all the answers

What do you call the elements in Groups 3-11?

Transition elements Signup and view all the answers

What are the elements in Group 17 called?

Halogens Signup and view all the answers

What is the name of the elements in Group 18?

Noble Gases Signup and view all the answers

Define Periods in the periodic table.

Horizontal rows which differ in the number of electrons and have the same number of principal energy levels. Signup and view all the answers

Where are Metals located in the periodic table?

Left of the staircase Signup and view all the answers

Where are Non-Metals located in the periodic table?

Right of the staircase Signup and view all the answers

What is Ionization Energy?

The energy needed to remove an electron from an atom. Signup and view all the answers

What are Metalloids?

Elements touching the staircase that have properties of both metals and non-metals. Signup and view all the answers

What gases are found on the periodic table?

H, N, O, F, Group 18 (A) Signup and view all the answers

Diatomic elements come in pairs.

True (A) Signup and view all the answers

Which elements are classified as Liquid Elements?

Br and Hg Signup and view all the answers

What elements are classified as Solid Elements?

All other elements that are not liquids, gases, or metalloids. Signup and view all the answers

Define Electronegativity.

The attraction of an atom for electrons. Signup and view all the answers

How does electronegativity change down a group?

Decreases (A) Signup and view all the answers

How does electronegativity change across a period from left to right?

Increases (B) Signup and view all the answers

Which element has the highest electronegativity?

F (4.0) Signup and view all the answers

How does ionization energy change down a group?

Decreases (D) Signup and view all the answers

How does ionization energy change across a period?

Increases (B) Signup and view all the answers

What is the definition of atomic radius?

Half the distance between adjacent nuclei. Signup and view all the answers

How does atomic radius change down a group?

It gets bigger because the number of principal energy levels increases. Signup and view all the answers

How does atomic radius change across a period from left to right?

It gets smaller due to increased nuclear charge pulling electrons closer. Signup and view all the answers

Define Conservation of Energy.

Energy cannot be created or destroyed; it changes from one form to another. Signup and view all the answers

Define Solubility.

The ability of a substance to dissolve in water. Signup and view all the answers

Study Notes

Father of the Periodic Table

Mendeleev is recognized as the father of the periodic table for his pioneering work in organizing elements.

Modern Periodic Table

The modern periodic table was developed by Mosley, focusing on atomic numbers.

Periodic Law

Elements are arranged by increasing atomic number.
Elements in the same group exhibit similar chemical properties.

Groups

Vertical columns in the periodic table.
Elements within a group react similarly due to having the same number of valence electrons.
Groups may contain a different number of principal energy levels (PEL).

Alkali Metals

Group 1 elements are known as alkali metals.

Alkaline Earth Metals

Group 2 elements are referred to as alkaline earth metals.

Transition Elements

Groups 3 to 11 are categorized as transition elements.

Halogens

Group 17 elements are identified as halogens.

Noble Gases

Group 18 consists of noble gases, characterized by having a complete set of 8 valence electrons.

Periods

Horizontal rows in the periodic table, with a total of 7 periods.
Each period represents a different number of electrons, with the same number of PELs.

Metals

Found to the left of the staircase line on the periodic table.
Metals have low ionization energy and tend to lose electrons, forming positive ions.
Excellent conductors of heat and electricity.

Non-Metals

Located to the right of the staircase.
Non-metals possess high ionization energy and electronegativity, making them poor conductors of heat and electricity.
Generally brittle and may shatter.

Ionization Energy

Defined as the energy required to remove an electron from an atom.
Having more valence electrons makes it increasingly difficult to remove an electron.
Noble gases in group 18 (with 8 valence electrons) resist losing electrons.

Metalloids

Elements that border the staircase, displaying properties of both metals and non-metals.
Notable metalloids include Boron (B), Silicon (Si), Arsenic (As), Tellurium (Te), Germanium (Ge), and Antimony (Sb).

Gases on the Periodic Table

Hydrogen (H), Nitrogen (N), Oxygen (O), and Fluorine (F) are diatomic gases, along with the noble gases in group 18.

Diatomic Elements

Certain elements exist as diatomic molecules, pairing with themselves: H, N, O, and F.

Liquid Elements

Bromine (Br) and Mercury (Hg) are the only elements that are liquid at room temperature.

Solid Elements

All other elements that are not classified as liquids or gases, including metalloids.

Electronegativity

Describes an element's tendency to attract electrons in a chemical bond.

Electronegativity Trends

Electronegativity decreases down a group as the atomic size increases.
Electronegativity increases across a period from left to right due to higher nuclear charge.

Highest Electronegativity

Fluorine (F) possesses the highest electronegativity value of 4.0.

Ionization Energy Trends

Ionization energy decreases down a group due to increased atomic size.
Ionization energy increases across a period from left to right as nuclear charge increases.

Atomic Radius

Defined as half the distance between adjacent nuclei of two atoms.

Atomic Radius Trends

The atomic radius increases down a group as additional principal energy levels (PEL) are added.
The atomic radius decreases across a period from left to right due to the increased nuclear charge pulling electrons closer.

Conservation of Energy

Energy cannot be created or destroyed; it merely transforms from one form to another.

Solubility

The ability of a substance to dissolve in water, indicating its interactions at the molecular level.

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Description

Test your knowledge of the periodic table with these flashcards focusing on key terms and concepts from the chapter. Learn about Mendeleev's contributions, the modern periodic table, and the periodic law, including the arrangement of elements. Perfect for reinforcing your understanding of the essential elements of chemistry.