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Grade 11 Chemistry Module 2: Chemical and Metallic Bonding
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Grade 11 Chemistry Module 2: Chemical and Metallic Bonding

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Questions and Answers

Define electron configuration.

The distribution of electrons among the orbitals of an atom.

Draw the electron configuration of the following using the s, p, d, and f: a) Na b) Ca c) Cl d) Zn e) F f) Al

a) Na: 1s^2 2s^2 2p^6 3s^1 b) Ca: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 c) Cl: 1s^2 2s^2 2p^6 3s^2 3p^5 d) Zn: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 e) F: 1s^2 2s^2 2p^5 f) Al: 1s^2 2s^2 2p^6 3s^2 3p^1

What is the smallest particle of an element?

Atom

What determines the atomic number of an element?

<p>Number of protons (also number of electrons)</p> Signup and view all the answers

What is the sum of an atom's protons and neutrons called?

<p>Mass number</p> Signup and view all the answers

Is the total number of protons in a given atom equal to the atomic number of the element?

<p>True</p> Signup and view all the answers

In which state can ions conduct electricity?

<p>molten</p> Signup and view all the answers

Why do ionic compounds not conduct electricity in their solid state?

<p>Ions are fixed in the crystal lattice</p> Signup and view all the answers

Covalent bonding involves the __________ of molecules.

<p>formation</p> Signup and view all the answers

Covalent compounds can have higher melting points than ionic compounds.

<p>False</p> Signup and view all the answers

Match the following allotropes of carbon with their properties:

<p>Diamond = Hard, transparent, non-conductor of heat and electricity Graphite = Soft, good conductor of heat and electricity, opaque</p> Signup and view all the answers

What is the charge of a proton?

<p>1+</p> Signup and view all the answers

What is the charge of an electron?

<p>1-</p> Signup and view all the answers

Which particle has almost zero mass?

<p>Electron</p> Signup and view all the answers

Protons + Neutrons = Atomic _______ Number

<p>Mass</p> Signup and view all the answers

What is the formula to find the total number of electrons in an energy level?

<p>number of electrons = 2n^2</p> Signup and view all the answers

What is the other name for the Group I elements?

<p>Alkali metals</p> Signup and view all the answers

What is the total number of protons in the nucleus of an atom?

<p>protons</p> Signup and view all the answers

Which statement is TRUE about the arrangement of elements in a periodic table?

<p>Atoms get larger going down a group.</p> Signup and view all the answers

Explain why the noble gases are unreactive.

<p>Noble gases are unreactive because they have a stable electronic configuration with 8 electrons in their outermost shell, except for helium which has 2 electrons.</p> Signup and view all the answers

What is the electron attracting ability to an atom called?

<p>electron affinity</p> Signup and view all the answers

Draw the atomic structure of the following elements and identify what group and period they belong: a) Zn

b) Al

c) F

Group______ period ______

<p>a) Group 12, Period 4 b) Group 13, Period 3 c) Group 17, Period 2</p> Signup and view all the answers

Name the ions present in sodium chloride: i. ____, ii. ____

Signup and view all the answers

What are atoms made of?

<p>protons, neutrons, electrons</p> Signup and view all the answers

What is the octet rule in chemical bonding?

<p>The octet rule states that atoms tend to gain, lose, or share electrons in order to have a full outer shell with 8 electrons, like the noble gases.</p> Signup and view all the answers

Explain the formation of sodium chloride (NaCl) using the ionic bond.

<p>Sodium (Na) donates its outer electron to chlorine (Cl) forming Na+ and Cl- ions, creating an ionic bond in sodium chloride (NaCl).</p> Signup and view all the answers

What makes one type of atom different from another?

<p>number of protons</p> Signup and view all the answers

What are the sub-particles found inside the atom? (Select all that apply)

<p>Neutrons</p> Signup and view all the answers

What property best describes ionic compounds?

<p>High melting and boiling points</p> Signup and view all the answers

Complete the table (by showing their masses and charge.)

<p>Proton: 1+ and 1; Neutron: 0 and 1; Electron: 1- and 0 (almost)</p> Signup and view all the answers

Give the number of protons, electrons, and neutrons in the atom below:

<p>a) N - Protons: 7, Electrons: 7, Neutrons: 7; b) K - Protons: 19, Electrons: 19, Neutrons: 20; c) Ne - Protons: 10, Electrons: 10, Neutrons: 10</p> Signup and view all the answers

Define Isotope:

<p>atom of the same element with the same number of protons but different number of neutrons</p> Signup and view all the answers

Define Mass spectrometer:

<p>instrument that separates isotopes and determines the mass of each isotope relative to the relative abundance of the isotopes</p> Signup and view all the answers

Calculate the relative atomic mass of Cu with 69% 63Cu and 31% 65Cu:

<p>63.2</p> Signup and view all the answers

Calculate the relative atomic mass of O with 99.79% 16O, 0.04% 17O, and 0.20% 18O:

<p>16.00</p> Signup and view all the answers

Define the term Atom?

<p>Atom is the basic unit of matter, consisting of a nucleus containing protons and neutrons, surrounded by electrons.</p> Signup and view all the answers

Define the term Atomic mass?

<p>Atomic mass is the average mass of an atom of an element, taking into account the isotopes and their relative abundances.</p> Signup and view all the answers

Define the term Atomic number?

<p>Atomic number is the number of protons in the nucleus of an atom, determining the identity of an element.</p> Signup and view all the answers

In what year was the neutron discovered?

<p>1932</p> Signup and view all the answers

Who discovered the electron?

<p>J.J. Thomson</p> Signup and view all the answers

Define the term Metalloid?

<p>Metalloid is an element that has properties that are between those of metals and nonmetals.</p> Signup and view all the answers

Define Ionization energy?

<p>Ionization energy is the energy required to remove an electron from an isolated atom or ion in the gaseous state.</p> Signup and view all the answers

Define Electron affinity?

<p>Electron affinity is the energy change that occurs when an atom gains an electron to form a negative ion.</p> Signup and view all the answers

Define Electronegativity?

<p>Electronegativity is the ability of an atom to attract and hold onto electrons in a chemical bond.</p> Signup and view all the answers

What are the two distinct trends in the atomic radius of elements in the periodic table?

<ol> <li>Atomic radius increases as you move down a group. 2. Atomic radius decreases as you move across a period.</li> </ol> Signup and view all the answers

How are elements arranged in the periodic table?

<p>Elements are arranged by increasing atomic number and atomic mass. They are grouped into periods (rows) and groups (columns) based on similar properties.</p> Signup and view all the answers

Which of the following statements describe the total number of protons in the nucleus of an atom? (Select all that apply)

<p>The total number of protons in the nucleus of an atom</p> Signup and view all the answers

In 1932, who proposed the atomic model involving electrons orbiting the nucleus in specific energy levels?

<p>Neil's Bohr</p> Signup and view all the answers

True or False: Atoms get larger going down a group.

<p>True</p> Signup and view all the answers

True or False: Atoms get smaller moving from left to right across each period.

<p>True</p> Signup and view all the answers

Elements are arranged from the lightest to ____.

<p>heaviest</p> Signup and view all the answers

What is the reason why atoms in the alkali group already have a stable outermost electron shell?

<p>Because their atoms have already have a stable outermost electron shell.</p> Signup and view all the answers

Name one ion present in sodium chloride besides sodium.

<p>Chloride</p> Signup and view all the answers

How many ions are present in sodium chloride?

<p>2</p> Signup and view all the answers

What is the electron attracting ability to an atom?

<p>The energy required to remove the outer electron from an isolated atom</p> Signup and view all the answers

Study Notes

Chemical and Metallic Bonding

  • The module is about chemical and metallic bonding, and it will take 10 weeks to complete.
  • The learning outcomes include:
    • Understanding the patterns of arrangement of electrons in atoms
    • Describing the electron arrangement in terms of shells and subshells
    • Explaining trends and relationships between elements in terms of atomic structure and bonding
    • Differentiating between ionic, covalent, and metallic bonds

Atomic Structure

  • An atom is the smallest particle of an element
  • Atoms of different elements may combine into systems called molecules
  • The nucleus is the small, dense core of an atom, composed of:
    • Protons (positively charged particles)
    • Neutrons (particles with no charge)
  • Electrons are negatively charged particles that orbit around the nucleus
  • The atomic number is the number of protons in an atom, which determines the element
  • The atomic mass or mass number is the sum of protons and neutrons in an atom

Atomic Models

  • Different models of atomic structure include:
    • The Rutherford model
    • The Bohr model
    • The Quantum Mechanical model

Protons, Neutrons, and Electrons

  • Protons:
    • Have a positive charge
    • Are found in the nucleus
    • Have a mass of 1 atomic mass unit (amu)
  • Neutrons:
    • Have no charge
    • Are found in the nucleus
    • Have a mass of 1 amu
  • Electrons:
    • Have a negative charge
    • Orbit around the nucleus
    • Have a negligible mass (almost 0 amu)

Atomic Number and Mass Number

  • The atomic number is the number of protons in an atom
  • The mass number is the sum of protons and neutrons in an atom
  • The number of neutrons can be calculated by subtracting the atomic number from the mass number

Relative Atomic Mass

  • Relative atomic mass (R.A.M) is a scale that compares the masses of atoms
  • The lightest element, hydrogen, has a mass of 1 on this scale
  • The R.A.M of an element is the average mass of its naturally occurring isotopes

Isotopes

  • Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons
  • Isotopes of an element have the same atomic number but different mass numbers
  • Examples of isotopes include carbon-12, carbon-13, and carbon-14

Relative Isotopic Mass

  • Relative isotopic mass is the mass of an atom of an isotope relative to the mass of an atom of 12C
  • It is a way to compare the masses of different isotopes### Isotopes and Atomic Mass
  • Isotopes of an element have different mass numbers but the same atomic number.
  • The relative atomic mass of an element is the weighted average of the masses of its isotopes.
  • A mass spectrometer is an instrument that separates the isotopes of an element and determines their relative abundance.

Electron Configuration

  • Electron configuration is the distribution of electrons in an atom's orbitals.
  • The electron configuration of an atom is represented by the number of electrons in each energy level.
  • The orbital's are represented by the letters s, p, d, and f.
  • The number of electrons in each orbital is determined by the formula: 2n^2.

Electron Shells

  • Electron shells are the energy levels of an atom where electrons are arranged.
  • The first shell can hold up to 2 electrons, the second shell can hold up to 8 electrons, and so on.
  • The electron configuration of an atom is represented by the number of electrons in each energy level.

Periodic Table

  • The periodic table is a chart of all the known elements in order of increasing atomic number.
  • The periodic table is divided into periods (rows) and groups (columns).
  • Elements in the same group have similar properties.
  • Elements in the same period have the same number of electron shells.

Development of the Periodic Table

  • The development of the periodic table began with John Dalton's atomic theory.
  • Johann Wolfgang Döbereiner discovered the triads of elements.
  • John Alexander Reina Newlands proposed the law of octaves.
  • Mendeleev's version of the periodic table is the most widely used today.

Atomic Number and Atomic Mass

  • The atomic number of an atom is the number of protons in the nucleus.
  • The atomic mass of an atom is the sum of the protons and neutrons in the nucleus.

Elements in the Periodic Table

  • Elements are named after their discoverer, place of discovery, or Latin name.
  • Elements are grouped into metals, non-metals, and metalloids.
  • Metals are lustrous, malleable, and ductile, and are found on the left side of the periodic table.
  • Non-metals are found on the upper right side of the periodic table.
  • Metalloids possess the properties of both metals and non-metals.
  • Atomic radius increases as you move down a group and decreases as you move across a period.
  • Ionization energy is the energy needed to remove an electron to form a positive ion.
  • Electron affinity is the energy change that occurs when an atom gains an electron to form a negative ion.
  • Electronegativity is a measure of an atom's attraction for electrons in a chemical bond.### Sublevels and Energy Levels
  • The s, p, d, and f are called sublevels, which are smaller subdivisions of energy within primary levels.
  • Each primary level has one more sublevel than the one below, with the first primary level having only s.
  • Sublevels are used to describe different energy levels, such as 3p or 3d.
  • Elements are arranged in the periodic table based on their properties.
  • The periodic table is full of repeating patterns, such as atomic size, which increases as you move down a group or period.
  • There are two distinct trends in the atomic radius of elements in the periodic table:
    • Atoms get larger going down a group (vertical arrangement or column).
    • Atoms get smaller moving from left to right across a period.

Ionization Energy, Electronegativity, and Electron Affinity

  • Ionization energy is the energy required to remove an outer electron from an isolated atom.
  • Electron affinity is the energy released when a neutral atom gains an extra electron to form a negatively charged ion.
  • Electronegativity is the electron-attracting ability of an atom.
  • The atomic radius is affected by ionization energy, electronegativity, and electron affinity, which increase from left to right across a period, causing the atomic radius to decrease.

Electron Configuration

  • Electron configuration is a way to describe the arrangement of electrons in an atom.
  • The table below shows the electron configuration of various elements, including their group and period numbers.

Groups and Periods

  • The periodic table is divided into groups (vertical columns) and periods (horizontal rows).
  • Elements are grouped according to their metals, nonmetals, and metalloids.
  • Metals are solid, malleable, ductile, and good conductors of heat, with a few exceptions.
  • Nonmetals can be solids, liquids, or gases, and are poor conductors of heat.
  • Metalloids are in-between metals and nonmetals, and have some properties of both.

Group I - The Alkali Metals

  • Group I elements are soft, silvery metals that react strongly with water.
  • The further down the group you go, the more violent this reaction is.
  • Alkali metals have one electron in their outer shells, and lose this electron to achieve a stable electron structure.

Group II - The Alkaline Earth Metals

  • Group II elements are metals that occur naturally in compound form.
  • They are less reactive than alkali metals.

Group III - The Aluminum Group

  • Group III elements are fairly reactive.
  • The group is composed of four metals and one metalloid.

Group IV - The Carbon Group

  • Group IV elements have varied properties, with their metallic property increasing from top to bottom.
  • The group is composed of metals, nonmetals, and metalloids.

Group V - The Nitrogen Group

  • Group V elements have varied properties, with some being metals, nonmetals, and metalloids.

Group VI - The Oxygen Group

  • Group VI elements are composed of nonmetals, metalloids, and metals.

Group VII - The Halogens

  • Group VII elements are entirely nonmetals.
  • The term halogen comes from the Greek words "hals" meaning salt and "genes" meaning forming.

Group VIII - The Noble Gases

  • Group VIII elements are stable gases, also known as inert or non-reactive elements.
  • They are unreactive due to their stable electronic configuration.

Bonding and Structure

  • Chemical bonds are formed when atoms combine to achieve a stable electronic configuration.
  • The octet rule explains the chemical bonding in many compounds, where atoms tend to attain a configuration with 8 electrons in their outermost shells.
  • There are two main types of chemical bonds:
    • Ionic bond: formed by the transfer of electrons from a metal to a non-metal.
    • Covalent bond: formed by the sharing of electrons between atoms.

Ionic Bond

  • The chemical bond formed by the transfer of electrons from a metal to a non-metal is known as an ionic or electrovalent bond.
  • Ionic bonds are formed when a metal atom loses an electron to become a positively charged cation, and a non-metal atom gains an electron to become a negatively charged anion.
  • The electrostatic attraction between the oppositely charged ions holds them together.

Properties of Ionic Compounds

  • Ionic compounds have high melting and boiling points due to the strong electrostatic forces of attraction between the ions.
  • Ionic compounds are crystalline solids, hard, and brittle.
  • Ionic compounds conduct electricity in their molten state and in aqueous solutions.
  • In solid state, ionic compounds do not conduct electricity due to the fixed positions of the ions in the crystal lattice.

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This quiz covers the topics of chemical and metallic bonding in Grade 11 Chemistry Module 2. It assesses the student's understanding of the concepts and principles of bonding in chemistry.

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