Periodic Table & Chemical Elements Quiz

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Questions and Answers

What is the common characteristic of alkaline earth metals in terms of their valence electrons?

Alkaline earth metals have two valence electrons.

How do halogens fill their outer electron shells?

Halogens gain one electron to fill their outer electron shells.

What defines the reactivity of noble gases?

Noble gases are unreactive due to having completely filled electron shells.

What happens to atomic radii as you move from top to bottom in the periodic table?

Atomic radii increase as you move from top to bottom in the periodic table. Signup and view all the answers

What are elements in Group 17 of the periodic table called, and what unique feature do they have?

Elements in Group 17 are called halogens, and they have seven valence electrons. Signup and view all the answers

What defines the concept of atomic radius in a diatomic molecule?

Atomic radius is defined as one-half the distance between the centers of two atoms in a homonuclear diatomic molecule. Signup and view all the answers

What trend is observed in ionization energy as you move across the periodic table?

Ionization energy generally increases as you move from left to right across the periodic table. Signup and view all the answers

Explain the significance of the filled electron shells in noble gases.

The filled electron shells in noble gases contribute to their chemical inertness. Signup and view all the answers

What does Mendeleev's Periodic Law state regarding the properties of elements?

It states that properties of elements are periodic functions of their atomic mass. Signup and view all the answers

How did Mendeleev predict the properties of unknown elements?

He left gaps in his table to represent the unknown elements and predicted their properties based on the properties of surrounding elements. Signup and view all the answers

What distinguishes the Modern Periodic Law from Mendeleev’s original periodic law?

The Modern Periodic Law states that properties repeat based on increasing atomic number, rather than atomic mass. Signup and view all the answers

What is the significance of noble gases in relation to Mendeleev's Periodic Table?

Noble gases were later discovered and could be placed in a separate group without disrupting the existing order of Mendeleev's table. Signup and view all the answers

Identify the elements classified as Alkali Metals in the periodic table.

The Alkali Metals include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr). Signup and view all the answers

In what manner are the elements arranged in the Modern Periodic Table?

They are arranged in a grid of 18 columns (groups) and 7 rows (periods), with a double row of elements below the main table. Signup and view all the answers

What chemical property do Barium (Ba) and Sodium (Na) share when compared to other elements?

Both Barium and Sodium can form ions, illustrating their chemical reactivity based on their position in the periodic table. Signup and view all the answers

Why was the discovery of noble gases important for the periodic table?

Their discovery confirmed the existence of properties that could be categorized without altering the arrangement of existing elements. Signup and view all the answers

What trend is observed in atomic size as you move from left to right across a period, and why does this occur?

Atomic size decreases from left to right due to increasing nuclear charge without a corresponding increase in electron shielding, pulling valence electrons closer to the nucleus. Signup and view all the answers

How does the ionic size of a cation compare to its neutral atom, and why?

A cation is smaller than its neutral atom because losing an electron reduces electron-electron repulsion and eliminates the outermost shell. Signup and view all the answers

Explain why Mg is larger than Mg++ while considering the charges involved.

Mg is larger than Mg++ because upon losing two electrons to form Mg++, the increased effective nuclear charge attracts the remaining electrons more strongly, reducing the size. Signup and view all the answers

What is the difference in size between anions and their neutral atoms, and what causes this difference?

Anions are larger than their neutral atoms due to the addition of electrons, which increases electron-electron repulsion and pushes the electrons further apart. Signup and view all the answers

Describe the relationship between ionization energy and atomic size trends across a period.

Ionization energy generally increases across a period as atomic size decreases, leading to stronger nuclear attraction making it harder to remove an electron. Signup and view all the answers

How does the coulombic law relate to atomic size? Provide the formula.

Coulombic law shows that atomic size is affected by the attraction between charged particles, represented by the formula: Fα q1q2/r². Signup and view all the answers

What trend is observed for ionic size when comparing anions to their respective neutral atoms?

Ionic size of anions is larger than their neutral atoms due to an increase in negative charge and resulting electron-electron repulsion. Signup and view all the answers

Why does atomic size increase down a group in the periodic table?

Atomic size increases down a group because additional electron shells are added, which outweighs the effect of increased nuclear charge. Signup and view all the answers

How does the size of an atom affect its ionization energy?

The ionization energy increases as the size of the atom decreases because valence electrons are closer to the nucleus and harder to remove. Signup and view all the answers

What role does electron shielding play in ionization energy trends within a group?

Electron shielding reduces the effective nuclear charge felt by valence electrons, leading to a decrease in ionization energy from top to bottom in a group. Signup and view all the answers

Why does nitrogen have a higher ionization potential than carbon or oxygen?

Nitrogen has a higher ionization potential due to its half-filled p subshell, providing extra stability compared to carbon and oxygen. Signup and view all the answers

What is electron affinity, and how is it related to an atom's propensity to gain an electron?

Electron affinity is the energy released when a neutral atom gains an electron; a more negative value indicates a higher tendency to attract electrons. Signup and view all the answers

How does the electron affinity trend change as you move down a group in the periodic table?

Electron affinity generally becomes less negative as you move down a group due to increased atomic size and electron-electron repulsions. Signup and view all the answers

Explain the trend of electron affinity across a period in the periodic table.

Electron affinity becomes more negative across a period because the atomic size decreases, enhancing the nucleus's attraction for added electrons. Signup and view all the answers

Define electronegativity and its significance in covalent bonds.

Electronegativity measures an atom's ability to attract electrons in a covalent bond and determines bond polarity. Signup and view all the answers

How does the octet rule influence electron affinity trends across a period?

The octet rule drives the increase in electron affinity across a period as elements become more stable when achieving a full valence shell. Signup and view all the answers

How does electronegativity change across a period and down a group?

Electronegativity increases across a period and decreases down a group. Signup and view all the answers

What is the relationship between atomic radius and electronegativity as one moves down a group?

As atomic radius increases down a group, electronegativity decreases because the valence electrons are farther from the nucleus. Signup and view all the answers

How does the bond strength relate to melting points of elements?

Stronger bonds require more energy to break, leading to higher melting points for those elements. Signup and view all the answers

Explain how metallic character varies across a period and down a group.

Metallic character decreases across a period and increases down a group. Signup and view all the answers

Define non-metallic character and its trend in the periodic table.

Non-metallic character is the tendency of an element to gain electrons and increases across a period but decreases down a group. Signup and view all the answers

What are metalloids and provide two examples?

Metalloids exhibit properties of both metals and non-metals; examples include Boron and Silicon. Signup and view all the answers

What happens to the energy required to gain electrons as you move from left to right across a period?

The energy required to gain electrons decreases as elements become more electronegative. Signup and view all the answers

Why is the process of losing electrons easier for elements as you descend a group?

Losing electrons becomes easier down a group due to increased atomic size, which means outer electrons are farther from the nucleus. Signup and view all the answers

Study Notes

Periodic Table & Library of Chemical Elements

The periodic table was organized by Dimitri Mendeleev, a Russian scientist.
Mendeleev classified elements based on increasing atomic mass and similar chemical properties.
The periodic table can be used to predict properties of new elements.
New elements discovered later fit right into the periodic table.

Modern Periodic Law

The Modern Periodic Law states the physical and chemical properties of elements repeat in a pattern when ordered by increasing atomic number (Z).
This law was proposed by Moseley.
Similar properties are observed at regular intervals on the periodic table.

Modern Periodic Table

The modern periodic table is arranged in a grid of 18 columns (groups/families) and 7 rows (periods).
There is also a double row of elements below the main grid.

Alkali Metals

Alkali metals reside in group 1 of the periodic table.
Examples of alkali metals include Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Caesium (Cs), Francium (Fr).
Alkali metals have one valence electron which is easily lost, forming a single positive charge ion.

Alkaline Earth Metals

Alkaline earth metals are located in group 2 of the periodic table.
Examples include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), and Radium (Ra).
These elements have two valence electrons and lose both to form ions with a two-plus charge.

Halogens

Halogens reside in group 17 of the periodic table.
These elements are Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At).
Halogens contain seven valence electrons and gain one electron to form singly-charged negative ions.

Noble Gases

Noble gases reside in group 18 of the periodic table.
They are Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), and Radon (Rn).
These elements are non-metals and possess completely filled electron shells, making them chemically unreactive.

Periodic Trends in the Table

There are clear trends in properties across the periodic table.
Trends include Atomic Radii, Ionic Radii, Ionization Potential/Energy, Electron Affinity, Electronegativity, Melting Point, Metallic/Non-Metallic Character.

Atomic Radii (Size) / Ionic Radii

Atomic radius is half the distance between the centers of two atoms in a homonuclear diatomic molecule.

Atomic Size

Atomic size increases from top to bottom due to the increasing number of electron shells.
Atomic size decreases from left to right due to increasing nuclear charge.

Ionic Size

Cations (positively charged ions) are smaller than the atom itself. This is because electron loss reduces the electron cloud, resulting in stronger nuclear attraction.
Anions (negatively charged ions) are larger than the neutral atom due to increased electron-electron repulsion, which pushes the electrons further apart.

Ionization Energy/Potential

Ionization energy is the energy needed to remove the most loosely bound valence electron.
Ionization energy increases from left to right (due to increasing nuclear charge) but decreases from top to bottom (due to increasing electron shielding and larger atomic size).

Electron Shielding

Electron shielding is the ability of inner electrons to shield outer valence electrons from the nucleus.

Electron Affinity

Electron affinity is the energy change when an atom gains an electron.
More negative values indicate higher affinity for electrons.
Electron affinity decreases going down a group (due to larger size).
Electron affinity increases across a period (due to increasing nuclear charge).

Electronegativity

Electronegativity is the tendency of an atom to attract electrons in a covalent bond.
Electronegativity increases from left to right (higher nuclear attraction) and decreases from top to bottom (due to larger size).

Melting Point

Melting point generally increases with stronger bonds.
Metals typically have high melting points.
Non-metals generally have low melting points.

Metallic Character

Metallic Character is the tendency of an element to lose electrons and form positive ions (cations).
Metallic character decreases across a period (due to a decrease in atomic size and increasing nuclear charge).
Metallic character increases down a group (due to increasing atomic size and weaker nuclear attraction).

Non-Metallic Character

Non-metallic character is the tendency of an element to gain electrons and form negative ions (anions).
Non-metallic character increases across a period, the opposite of metallic character.
Non-metallic character decreases down a group.

Metalloids

Metalloids are elements that exhibit both metal and non-metal properties.
Examples include Boron (B), Silicon (Si), and Arsenic (As).

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Description

Test your knowledge on the periodic table, its organization, and the Modern Periodic Law. Discover how elements are classified and learn about alkali metals and their properties. This quiz covers essential concepts from chemistry related to the periodic table.