The document outlines the curriculum for several terms, including the units that will be covered in chemistry such as Unit 2 on chemistry and the universe. It provides learning objectives and topics that will be studied for Unit 2, including atomic structure, ionic and covalent bonding, and the properties of different elements and compounds. A practical activity is described where students will investigate the properties of elements.
The document outlines a chemistry curriculum covering various units over 3 terms, including topics like atomic structure, ionic and covalent bonding, and properties of substances. It provides learning objectives and details on unit 2 which will cover chemical reactivity and bonding, properties based on chemical structure, and factors affecting chemical reactions. The unit will involve learning atomic structure, ionic and covalent bonding through activities like drawing dot and cross diagrams.
Electrons and chemical bonding spring 2014 day 1jmori
The document provides instructions for students on an upcoming chemistry lesson, including materials needed, homework assignments, and review questions. Students are asked to create flashcards with chemistry questions and answers and will have a quiz on Friday covering topics like ionic and covalent bonding, electronegativity, and drawing Lewis dot diagrams. The lesson will focus on how chemical bonding allows elements to join together in different combinations and form new substances with different properties.
- Isotopes are atoms of the same element that have different numbers of neutrons. Some isotopes are radioactive while others are non-radioactive.
- Radioactive isotopes can be useful in medical applications like cancer treatment and dating ancient remains, as well as industrial uses like leak detection. Their half-lives determine how long it takes for half of a sample to decay.
- Atoms gain and lose electrons to form ions, and ionic bonds form between oppositely charged ions. Ionic compounds have high melting points and are usually soluble in water.
This document provides information on ionic compounds and metals. It discusses how ions are formed through the gain or loss of valence electrons to achieve stable octet configurations. Ionic compounds contain oppositely charged ions that are attracted to each other. Their crystal lattices give them high melting and boiling points. Metals form lattices with cations surrounded by a sea of delocalized electrons, giving them malleability, ductility, and high conductivity.
The document discusses chemical bonding, including the formation of ions, ionic bonds, metallic bonds, and covalent bonds. Ions are formed when atoms gain or lose electrons to obtain full outer electron shells. Ionic bonds form when ions of opposite charge attract via electrostatic forces. Metallic bonds occur via delocalized electrons within metal atoms. Covalent bonds form through the sharing of electron pairs between nonmetal atoms. The octet rule and electronegativity help explain bonding properties.
The document summarizes the key differences between ionic and covalent bonding. Ionic bonds form when a metal transfers electrons to a nonmetal, creating oppositely charged ions. Covalent bonds form when nonmetals share electrons to obtain a full outer shell. Ionic compounds have high melting points, are brittle solids, and dissolve well in water, while covalent compounds have lower melting points, are soft and pliable, and are generally insoluble in water.
Ionic compounds form when oppositely charged ions attract each other, forming ionic bonds. Ions are formed when atoms gain or lose valence electrons to achieve a stable electron configuration. In ionic compounds, the cation is written first followed by the anion in chemical formulas. Metals form metallic bonds where metal atoms donate their valence electrons, which are free to move throughout the crystal lattice structure.
The document outlines a chemistry curriculum covering various units over 3 terms, including topics like atomic structure, ionic and covalent bonding, and properties of substances. It provides learning objectives and details on unit 2 which will cover chemical reactivity and bonding, properties based on chemical structure, and factors affecting chemical reactions. The unit will involve learning atomic structure, ionic and covalent bonding through activities like drawing dot and cross diagrams.
Electrons and chemical bonding spring 2014 day 1jmori
The document provides instructions for students on an upcoming chemistry lesson, including materials needed, homework assignments, and review questions. Students are asked to create flashcards with chemistry questions and answers and will have a quiz on Friday covering topics like ionic and covalent bonding, electronegativity, and drawing Lewis dot diagrams. The lesson will focus on how chemical bonding allows elements to join together in different combinations and form new substances with different properties.
- Isotopes are atoms of the same element that have different numbers of neutrons. Some isotopes are radioactive while others are non-radioactive.
- Radioactive isotopes can be useful in medical applications like cancer treatment and dating ancient remains, as well as industrial uses like leak detection. Their half-lives determine how long it takes for half of a sample to decay.
- Atoms gain and lose electrons to form ions, and ionic bonds form between oppositely charged ions. Ionic compounds have high melting points and are usually soluble in water.
This document provides information on ionic compounds and metals. It discusses how ions are formed through the gain or loss of valence electrons to achieve stable octet configurations. Ionic compounds contain oppositely charged ions that are attracted to each other. Their crystal lattices give them high melting and boiling points. Metals form lattices with cations surrounded by a sea of delocalized electrons, giving them malleability, ductility, and high conductivity.
The document discusses chemical bonding, including the formation of ions, ionic bonds, metallic bonds, and covalent bonds. Ions are formed when atoms gain or lose electrons to obtain full outer electron shells. Ionic bonds form when ions of opposite charge attract via electrostatic forces. Metallic bonds occur via delocalized electrons within metal atoms. Covalent bonds form through the sharing of electron pairs between nonmetal atoms. The octet rule and electronegativity help explain bonding properties.
The document summarizes the key differences between ionic and covalent bonding. Ionic bonds form when a metal transfers electrons to a nonmetal, creating oppositely charged ions. Covalent bonds form when nonmetals share electrons to obtain a full outer shell. Ionic compounds have high melting points, are brittle solids, and dissolve well in water, while covalent compounds have lower melting points, are soft and pliable, and are generally insoluble in water.
Ionic compounds form when oppositely charged ions attract each other, forming ionic bonds. Ions are formed when atoms gain or lose valence electrons to achieve a stable electron configuration. In ionic compounds, the cation is written first followed by the anion in chemical formulas. Metals form metallic bonds where metal atoms donate their valence electrons, which are free to move throughout the crystal lattice structure.
I. Ionic compounds form when oppositely charged ions bond via ionic bonds. When atoms gain or lose electrons to achieve stable octet configurations, they form cations or anions that bond in a crystalline lattice.
II. Ionic bonds are strong electrostatic attractions between cations and anions. Ionic compounds have high melting and boiling points and are brittle solids that do not conduct electricity well.
III. Formulas and names of ionic compounds follow conventions where the cation is written first followed by the anion. Polyatomic ions are also considered when writing formulas and names.
Ionic bonds form when oppositely charged ions attract each other, forming ionic compounds. Cations form when atoms lose electrons to achieve a stable electron configuration, while anions form when atoms gain electrons. Ionic compounds consist of a crystal lattice structure where cations are surrounded by anions. They have properties like high melting points and boiling points since energy is required to overcome the strong electrostatic attractions between ions.
The document provides information about an upcoming Chemistry Midterm Exam, including:
- The exam is divided into 3 sections testing multiple choice, short answer, and mixed question types.
- Students should bring a calculator, pen, and pencil, as reference tables will be provided.
- The exam covers 12 topics such as matter and change, atomic structure, bonding, and chemical reactions.
- The purpose of the review packet is to highlight key ideas from the course that will be on the exam, and should be used along with other study materials to thoroughly prepare for the test. Active study is required to do well.
This document defines chemical formulas and explains how atoms form compounds. It states that a chemical formula tells what elements are in a compound and the number of atoms. It then discusses that atoms form compounds due to electric forces between protons and electrons. Atoms seek to gain or lose electrons to achieve a stable outer electron level. The document goes on to describe ionic and covalent bonds. Ionic bonds form when a metal transfers electrons to a nonmetal. Covalent bonds form when nonmetals share electrons. It provides examples of naming ionic and covalent compounds.
The document provides information about the Chemistry Midterm Exam, including its three sections and topics covered. It notes the exam allows one class period and a scientific calculator. The exam covers 12 topics such as matter and change, the periodic table, and chemical reactions. The purpose of the review packet is to help students prepare for the exam using key ideas from the core curriculum along with their own notes, review sheets, and reference tables. Active preparation is necessary as there are no shortcuts to passing.
The document discusses different types of chemical bonds including ionic bonds, polar covalent bonds, and nonpolar covalent bonds. It explains that ionic bonds form between metal and nonmetal atoms through the transfer of electrons from metals to nonmetals, creating positive and negative ions. Polar covalent bonds form when electrons are unequally shared between atoms. The polarity of a bond depends on the difference in electronegativity between the atoms. Metallic bonds involve the delocalization of electrons within a crystal lattice of positive ions.
Ionic bonding occurs when atoms transfer electrons to form charged ions. Metals react with non-metals, where the metal loses electrons and the non-metal gains electrons to form ions. These ions then bond together in a crystal lattice structure with an overall neutral charge. Covalent bonding occurs when non-metals share electron pairs to form molecules. Metallic bonding involves delocalized electrons that are attracted to the positively charged metal ions, binding them together in a giant lattice structure.
1. The document discusses periodic trends in atomic properties such as size, ionization energy, and electron affinity across the periodic table.
2. Key periodic trends described include decreasing atomic size and increasing ionization energy from left to right across a period, and decreasing ionization energy from top to bottom in a group.
3. Exceptions to trends are discussed, such as higher ionization energies for p-block versus s-block elements and for doubly-occupied versus singly-occupied orbitals.
1. Isotopes are atomic forms of the same element that have the same number of protons and electrons but a different number of neutrons.
2. Ionic bonding occurs when metals lose electrons to form positive ions, and non-metals gain electrons to form negative ions. Ionic compounds have high melting and boiling points.
3. Covalent bonding occurs when two non-metal atoms share electrons in their outer shell to complete their electron configuration. Covalent substances have low melting and boiling points.
1. Isotopes are atomic forms of the same element that have the same number of protons and electrons but a different number of neutrons.
2. Ionic bonding occurs when metals lose electrons to form positive ions, and non-metals gain electrons to form negative ions. Ionic compounds have high melting and boiling points.
3. Covalent bonding occurs when two non-metal atoms share electrons in their outer shell to complete their electron configuration. Covalent substances have low melting and boiling points.
The document provides instructions for a chemistry lesson that involves identifying elements and compounds, describing chemical bonding and ion formation, and balancing chemical equations. Students are asked to complete tasks using resources like the periodic table, textbooks, and online learning modules. They will learn about chemical bonding, ion formation, and the properties of ionic compounds by creating examples like sodium chloride. Questions are provided to test their understanding.
Electrons and chemical bonding spring 2014 day 2jmori
The document provides instructions for students to complete a STAR quiz and worksheet on chemical bonding. It includes the following key points:
1) Students need materials like a pencil, periodic table, and colored pencils for the worksheet.
2) They must turn in STAR cards and will be assigned a computer to continue the worksheet after the quiz.
3) The worksheet involves drawing Lewis dot diagrams, identifying ionic and covalent bonds, and calculating electronegativity.
4) Homework on ionic and covalent bonding is due next week along with completed STAR cards.
This document discusses chemical bonds and how they form compounds. It explains that ionic bonds form between metals and nonmetals when electrons are transferred, creating oppositely charged ions. Covalent bonds form when atoms share electrons. There are different types of covalent bonds depending on how electrons are shared. The document provides examples of naming simple ionic compounds and covalent molecules, and discusses more complex compounds involving polyatomic ions or water of hydration.
Ionic compounds are formed when ions bond via ionic bonds. Ions form when atoms gain or lose electrons to achieve a stable electron configuration. Ionic bonds result from the electrostatic attraction between oppositely charged ions. Ionic compounds consist of a crystal lattice structure where ions are arranged in a repeating pattern. Metals form metallic bonds where delocalized electrons are attracted to metallic cations. Alloys are mixtures of metals or metals with other elements that have distinct properties from their components.
1. The document provides a lesson plan and syllabus content for a chemistry lesson on atomic structure, elements, compounds, mixtures, and chemical bonding.
2. Key topics covered in the lesson include atomic structure, isotopes, the differences between elements, compounds and mixtures, ionic and covalent bonding, and the properties of ionic, covalent and metallic substances.
3. Homework assigned is to review the topic of chemical bonding covered in class.
The document summarizes key concepts about the structure of atoms and the nature of matter:
1) Atoms are made up of protons, neutrons, and electrons, with protons and neutrons located in the nucleus and electrons located outside the nucleus.
2) Isotopes of the same element have the same number of protons but different numbers of neutrons, and all isotopes of an element have the same chemical properties.
3) Compounds have different physical and chemical properties than their constituent elements due to the formation of chemical bonds between the elements.
According to Gilbert Lewis, atoms combine i order to achieve a more stable electron configuration. Maximum stability is obtained when an atom is isoelectronic with a noble gas. This presentation would enable students to relate lattice energy with physical properties such as melting point.
This document provides an overview of chemical bonding, including ionic and covalent bonds. It explains that ionic bonds form when ions transfer electrons, while covalent bonds form when atoms share electrons. The octet rule and Lewis electron dot diagrams are introduced to show how atoms gain or share electrons to achieve stable electron configurations like noble gases. Ionic compounds are formed from metals transferring electrons to nonmetals, resulting in cations and anions that bond ionically. Covalent compounds are formed by nonmetals sharing electrons in molecules. Molecular geometry is also discussed, including the shapes of molecules based on the number of electron pairs around the central atom.
The document discusses topics related to chemical reactions and the periodic table. It provides information on:
- Mendeleev's creation of the periodic table and how he arranged elements based on their properties.
- The structure of atoms consisting of protons, neutrons, and electrons located in electron shells around the nucleus.
- The modern periodic table including atomic number and mass number.
- Ionic bonding forming between metals and non-metals through the transfer of electrons. Ionic compounds have high melting/boiling points and conduct electricity when molten or dissolved.
- Covalent bonding forming when atoms share electrons in covalent molecules. Simple covalent substances have low melting/boiling points while giant
Electrons and Chemical Bonding spring 2014 day 2jmori
1) Students will take a 15 minute STAR quiz and then be assigned to computers to continue working on an electron and chemical bonding worksheet.
2) After the quiz, students should turn it in, return manilla folders, and sign out a computer from Mrs. M to work on the worksheet, making sure to use their own words, highlight important information, and review all pages.
3) The document provides information on chemical bonding and how atoms bond by sharing, gaining or losing electrons, and explains the characteristics of ionic and covalent bonds. Homework assigned is to complete the electron and chemical bonding worksheet by next week and to prepare STAR cards for the following class.
I. Ionic compounds form when oppositely charged ions bond via ionic bonds. When atoms gain or lose electrons to achieve stable octet configurations, they form cations or anions that bond in a crystalline lattice.
II. Ionic bonds are strong electrostatic attractions between cations and anions. Ionic compounds have high melting and boiling points and are brittle solids that do not conduct electricity well.
III. Formulas and names of ionic compounds follow conventions where the cation is written first followed by the anion. Polyatomic ions are also considered when writing formulas and names.
Ionic bonds form when oppositely charged ions attract each other, forming ionic compounds. Cations form when atoms lose electrons to achieve a stable electron configuration, while anions form when atoms gain electrons. Ionic compounds consist of a crystal lattice structure where cations are surrounded by anions. They have properties like high melting points and boiling points since energy is required to overcome the strong electrostatic attractions between ions.
The document provides information about an upcoming Chemistry Midterm Exam, including:
- The exam is divided into 3 sections testing multiple choice, short answer, and mixed question types.
- Students should bring a calculator, pen, and pencil, as reference tables will be provided.
- The exam covers 12 topics such as matter and change, atomic structure, bonding, and chemical reactions.
- The purpose of the review packet is to highlight key ideas from the course that will be on the exam, and should be used along with other study materials to thoroughly prepare for the test. Active study is required to do well.
This document defines chemical formulas and explains how atoms form compounds. It states that a chemical formula tells what elements are in a compound and the number of atoms. It then discusses that atoms form compounds due to electric forces between protons and electrons. Atoms seek to gain or lose electrons to achieve a stable outer electron level. The document goes on to describe ionic and covalent bonds. Ionic bonds form when a metal transfers electrons to a nonmetal. Covalent bonds form when nonmetals share electrons. It provides examples of naming ionic and covalent compounds.
The document provides information about the Chemistry Midterm Exam, including its three sections and topics covered. It notes the exam allows one class period and a scientific calculator. The exam covers 12 topics such as matter and change, the periodic table, and chemical reactions. The purpose of the review packet is to help students prepare for the exam using key ideas from the core curriculum along with their own notes, review sheets, and reference tables. Active preparation is necessary as there are no shortcuts to passing.
The document discusses different types of chemical bonds including ionic bonds, polar covalent bonds, and nonpolar covalent bonds. It explains that ionic bonds form between metal and nonmetal atoms through the transfer of electrons from metals to nonmetals, creating positive and negative ions. Polar covalent bonds form when electrons are unequally shared between atoms. The polarity of a bond depends on the difference in electronegativity between the atoms. Metallic bonds involve the delocalization of electrons within a crystal lattice of positive ions.
Ionic bonding occurs when atoms transfer electrons to form charged ions. Metals react with non-metals, where the metal loses electrons and the non-metal gains electrons to form ions. These ions then bond together in a crystal lattice structure with an overall neutral charge. Covalent bonding occurs when non-metals share electron pairs to form molecules. Metallic bonding involves delocalized electrons that are attracted to the positively charged metal ions, binding them together in a giant lattice structure.
1. The document discusses periodic trends in atomic properties such as size, ionization energy, and electron affinity across the periodic table.
2. Key periodic trends described include decreasing atomic size and increasing ionization energy from left to right across a period, and decreasing ionization energy from top to bottom in a group.
3. Exceptions to trends are discussed, such as higher ionization energies for p-block versus s-block elements and for doubly-occupied versus singly-occupied orbitals.
1. Isotopes are atomic forms of the same element that have the same number of protons and electrons but a different number of neutrons.
2. Ionic bonding occurs when metals lose electrons to form positive ions, and non-metals gain electrons to form negative ions. Ionic compounds have high melting and boiling points.
3. Covalent bonding occurs when two non-metal atoms share electrons in their outer shell to complete their electron configuration. Covalent substances have low melting and boiling points.
1. Isotopes are atomic forms of the same element that have the same number of protons and electrons but a different number of neutrons.
2. Ionic bonding occurs when metals lose electrons to form positive ions, and non-metals gain electrons to form negative ions. Ionic compounds have high melting and boiling points.
3. Covalent bonding occurs when two non-metal atoms share electrons in their outer shell to complete their electron configuration. Covalent substances have low melting and boiling points.
The document provides instructions for a chemistry lesson that involves identifying elements and compounds, describing chemical bonding and ion formation, and balancing chemical equations. Students are asked to complete tasks using resources like the periodic table, textbooks, and online learning modules. They will learn about chemical bonding, ion formation, and the properties of ionic compounds by creating examples like sodium chloride. Questions are provided to test their understanding.
Electrons and chemical bonding spring 2014 day 2jmori
The document provides instructions for students to complete a STAR quiz and worksheet on chemical bonding. It includes the following key points:
1) Students need materials like a pencil, periodic table, and colored pencils for the worksheet.
2) They must turn in STAR cards and will be assigned a computer to continue the worksheet after the quiz.
3) The worksheet involves drawing Lewis dot diagrams, identifying ionic and covalent bonds, and calculating electronegativity.
4) Homework on ionic and covalent bonding is due next week along with completed STAR cards.
This document discusses chemical bonds and how they form compounds. It explains that ionic bonds form between metals and nonmetals when electrons are transferred, creating oppositely charged ions. Covalent bonds form when atoms share electrons. There are different types of covalent bonds depending on how electrons are shared. The document provides examples of naming simple ionic compounds and covalent molecules, and discusses more complex compounds involving polyatomic ions or water of hydration.
Ionic compounds are formed when ions bond via ionic bonds. Ions form when atoms gain or lose electrons to achieve a stable electron configuration. Ionic bonds result from the electrostatic attraction between oppositely charged ions. Ionic compounds consist of a crystal lattice structure where ions are arranged in a repeating pattern. Metals form metallic bonds where delocalized electrons are attracted to metallic cations. Alloys are mixtures of metals or metals with other elements that have distinct properties from their components.
1. The document provides a lesson plan and syllabus content for a chemistry lesson on atomic structure, elements, compounds, mixtures, and chemical bonding.
2. Key topics covered in the lesson include atomic structure, isotopes, the differences between elements, compounds and mixtures, ionic and covalent bonding, and the properties of ionic, covalent and metallic substances.
3. Homework assigned is to review the topic of chemical bonding covered in class.
The document summarizes key concepts about the structure of atoms and the nature of matter:
1) Atoms are made up of protons, neutrons, and electrons, with protons and neutrons located in the nucleus and electrons located outside the nucleus.
2) Isotopes of the same element have the same number of protons but different numbers of neutrons, and all isotopes of an element have the same chemical properties.
3) Compounds have different physical and chemical properties than their constituent elements due to the formation of chemical bonds between the elements.
According to Gilbert Lewis, atoms combine i order to achieve a more stable electron configuration. Maximum stability is obtained when an atom is isoelectronic with a noble gas. This presentation would enable students to relate lattice energy with physical properties such as melting point.
This document provides an overview of chemical bonding, including ionic and covalent bonds. It explains that ionic bonds form when ions transfer electrons, while covalent bonds form when atoms share electrons. The octet rule and Lewis electron dot diagrams are introduced to show how atoms gain or share electrons to achieve stable electron configurations like noble gases. Ionic compounds are formed from metals transferring electrons to nonmetals, resulting in cations and anions that bond ionically. Covalent compounds are formed by nonmetals sharing electrons in molecules. Molecular geometry is also discussed, including the shapes of molecules based on the number of electron pairs around the central atom.
The document discusses topics related to chemical reactions and the periodic table. It provides information on:
- Mendeleev's creation of the periodic table and how he arranged elements based on their properties.
- The structure of atoms consisting of protons, neutrons, and electrons located in electron shells around the nucleus.
- The modern periodic table including atomic number and mass number.
- Ionic bonding forming between metals and non-metals through the transfer of electrons. Ionic compounds have high melting/boiling points and conduct electricity when molten or dissolved.
- Covalent bonding forming when atoms share electrons in covalent molecules. Simple covalent substances have low melting/boiling points while giant
Electrons and Chemical Bonding spring 2014 day 2jmori
1) Students will take a 15 minute STAR quiz and then be assigned to computers to continue working on an electron and chemical bonding worksheet.
2) After the quiz, students should turn it in, return manilla folders, and sign out a computer from Mrs. M to work on the worksheet, making sure to use their own words, highlight important information, and review all pages.
3) The document provides information on chemical bonding and how atoms bond by sharing, gaining or losing electrons, and explains the characteristics of ionic and covalent bonds. Homework assigned is to complete the electron and chemical bonding worksheet by next week and to prepare STAR cards for the following class.
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This Dissertation explores the particular circumstances of Mirzapur, a region located in the
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Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
structure of plant communities across different temporal and spatial scales. These changes can
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4. Unit Content
Learning aim A: Investigate chemical reactivity and bonding
Learning aim B: Investigate how the uses of chemical
substances depend on their chemical and physical properties
Learning aim C: Investigate the factors involved in the rate of
chemical reactions.
Learning aim D: Understand the factors that are affecting the
Earth and its environment
5. Learning Objectives:
1. Describe the physical and chemical properties of group
1 and 7 elements.
2. Describe trend in the physical and chemical properties
of group 1 and 7 elements.
3. Explain the trend in chemical properties in terms of
electronic structure.
4. Explain the formation of ionic and covalent substances
5. Compare and explain the properties of ionic & covalent
substances, and their applications.
Learning aim A: Investigate chemical reactivity and bonding
6. What we will study today?
• The atomic structure.
• Ionic and covalent bonding
– Properties
– Dot and cross diagram
• Practical – properties of elements.
7. Starter
• Label the atomic diagram
• Complete the fill in gap work sheet
• 10 min
11. The Atom: SomeFacts
• Atomsareneutral.Theyhaveno overall charge becausethe numberofprotonsandelectrons
arethe same.
Particle Relative Mass Relative Charge
proton 1 +1
neutron 1 0
electron very small -1
• Atomshavearadiusof0.1 nanometers.
12. Elements
Elements are made of one type of atom only.
Theyarerepresented bybothanameanda symbol.Forexample,
carbon= C andsodium= Na(noticehowthe firstletteris alwaysshownbyacapitalandthe
second is lowercase).
13. Elements
Lookatyourcopyofthe periodictable.Apartfromthe element nameandsymbol,whatelsedo
younotice?
Atomic Number
Mass Number
The atomic number is the number of
protons each atom contains.
The mass number is the total number of
protons and neutrons in the atom.
O
16
8
14. How many protons, electrons and
neutrons does fluorine have?
19
9
F
Atomic weight
Number of protons AND
neutrons
Atomic number
Number of protons
(Number of electrons too)
electron -
Proton +
Neutron 0
9
9
10
15. Atoms andElements Activity
Eachpersonwillbe given a cardwith a question on it. Each
card also has a questionnumber.
Read your questionand recordyour answeron the answer
sheetnextto the appropriatenumber.
Move around the room swapping questioncardswith other
pupils. Each timeyou swap a card, read the questionand
recordyour answer.
There are 30 questions in total.
How many can you complete in
10 minutes?
16.
17.
18. Making of Substances
There are millions of substances and all have different properties.
But why?
This is because:
They are made up of different elements
How they are held together (the bonding)
How they are arranged (the structure)
19. Substances and Molecules are produced by forming different types
of chemical bond.
In chemical bond, the electrons in the outer shell of the atoms are
rearranged by sharing or transferring.
When electrons are shared, it is called covalent bonding.
When electrons are transferred, it is called ionic bonding.
Making of Substances
20. Covalent bonding and substances
A covalent bond is only formed between two non-metal atoms by
sharing electrons.
The electrons shared are only from the outer shell – so no electrons
are lost or gained.
Covalent substance are either separate molecules, e.g. water; or giant
structure like diamond.
21. Types of covalent bonding
Single Covalent Bond
Double Covalent Bond
Quadrupole Covalent
Bond
22. Ionic bonding
When an atom, or a group of atoms lose or gain electrons to obtain full
outer shells, a new charged particle is formed – called Ions.
Ions from in reaction between a metal and a non-metal.
In the reaction:
the metal atoms lose electrons to form positively charged ions
the non-metal atoms gain electrons to form negatively charged ions
Ionic bonds are strong
electrostatic forces
between oppositely
charged ions
24. • The bonding between atoms in a covalent molecule is very strong.
• But, there are only very week forces/attraction between the two
molecules in a substance.
• So, simple covalent substances:
do not conduct electricity even when melted
have low melting and boiling point – so often gases or liquids
Not usually soluble in water, but may dissolve in organic solvent.
Properties of simple covalent substances
25. Properties of giant covalent substances
Do you know why diamond is the hardest natural substances? Why
diamond take thousands of year to form?
Diamond is made up of carbon, which has
four electrons in the outer shell.
So, it can form four covalent bonds, and
this structural bonding goes on and on
As a result, it forms a very strong
tetrahedral structure.
Thereby, it has very high melting and
billing points
Examples of giant covalent substance
include silica, polymer, graphite
26. Properties of Ionic substances
Does an sodium chloride (salt) molecule exist?
NO
Ions in a solid ionic substances are not
randomly arranged.
They have a regular, repeating arrangement
called an ionic lattice.
So, ionic compounds don’t form small
molecules, instead they form crystal with
regular shapes.
A sodium can surround itself with six chlorides
ions and vice versa – forming a giant ionic
structure.
Properties: high melting and boiling points,
conduct electricity & dissolve in water.
27. Useful Ionic bonds
Since ionic bonds are formed between positively charged and negatively
charged atoms, ionic compounds are strong and with regular structure.
Most of the earth’s rocks have ionic bonds.
As a result, the rocks are hard and durable.
They have high melting and boiling points – solid at RT
Ionic compounds conduct electricity when melted or in solution.
They are insulator when solid.
28. Activity
• Complete the table to summarise the properties
of ionic and covalent substances.
• 10 min
Property Covalent substances Ionic substances
Appearance
Solubility
Melting & boiling
points
Electrical
conductivity
29. Properties of ionic & covalent substances
Property Covalent substances Ionic substances
Appearance Solid, liquid or gas at room
temperature
Most are solid or
crystalline at room
temperature
Solubility Many dissolves in organic
solvents, but not in water
Dissolve in water, not in
organic solvent
Melting &
boiling points
Many have low melting and
boiling points
High melting and boiling
points
Electrical
conductivity
Do not conduct electricity Conduct electricity when
molten or dissolved
Discuss in your group to explain why the ionic and covalent substances
have these properties?
30. Activity
• Discuss in your group to explain why the ionic
and covalent substances have the properties.
• Write down your answer
32. Dot and Cross Diagrams
Dot and cross diagrams show the arrangement of the outer-shell
electrons in an ionic or covalent compound or element.
The electrons are shown as dots and crosses
In a dot and cross diagram:
Only the outer electrons are shown
The charge of the ion is spread evenly which is shown by using brackets
The charge on each ion is written at the top right-hand corner
33. Ionic
compounds
How to draw Dot and Cross Diagrams?
Covalent
compounds
Step 1: Draw the atoms with
their outer shell.
Step 2: Put the atoms together and
check they all have a full outer shell.
34. Example 1: water, H2O
Example 2: oxygen, O2:
O
H H
O O
H
H
O
O O
Step 1: Draw the atoms with
their outer shell.
Step 2: Put the atoms together and
check they all have a full outer shell.
Dot and cross diagrams
35. Activity
Draw dot-and-cross diagrams and write formulae
for the following:
• Covalent: hydrogen, chlorine, carbon dioxide, methane,
water, oxygen.
• Ionic: sodium chloride, magnesium oxide, magnesium
chloride.