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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Description

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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