3.1-3.7: Atoms, Elements and Compounds 

%%Atoms are the smallest particles of matter, that we cannot break down further by chemical means.%%

Elements Contain only one kind of atom, example sodium.

Defining Proton Number

• The atomic number (or proton number) is the number of protons in the nucleus of an atom
• The symbol for atomic number is Z
• It is also the number of electrons present in a neutral atom and determines the position of the element on the Periodic Table.

Defining Nucleon Number

• ^^Nucleon number (or mass number) is the total number of protons and neutrons in the nucleus of an atom^^

• The symbol for nucleon number is A

  how to find neutrons number: The nucleon number minus the proton number gives you the number of neutrons of an atom

• protons + neutrons are called nucleons.

• The atomic number and mass number for every element is on the Periodic Table

  

Electrons

• The symbol for an electron is e-, but other symbols are used such as x and ⦁ in bonding diagrams to make it easier to see where electrons come from.

• These subatomic particles move very fast around the nucleus.

• They move in orbital paths called shells

• The mass of the electron is negligible, hence the mass of an atom is concentrated in the nucleus where the neutrons and protons are found.

  

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Protons neutrons and elements

• ^^Elements are made of tiny particles of matter called atoms^^

• ^^Each atom is made of subatomic particles called protons, neutrons and electrons^^

• Their size is so tiny that we can't really compare their masses in conventional units such as kilograms or grams, so a unit called the relative atomic mass is used

• One relative atomic mass unit is equal to 1/12th the mass of a carbon-12 atom.

• All other elements are measured relative to the mass of a carbon-12 atom, so relative atomic mass has no units (although sometimes you may come across a unit Da or u which stands for a Dalton and it means the same thing).

• Hydrogen for example has a relative atomic mass of 1, meaning that 12 atoms of hydrogen would have exactly the same mass as 1 atom of carbon

• The relative mass and charge of the subatomic particles are shown below:

  

Types of Substances and there Properties

Compound

A pure substance made up of two or more elements chemically combined.

• There is an unlimited number of compounds
• Compounds cannot be separated into their elements by physical means.

example: Copper sulfate and calcium carbonate Mixture

• A combination of two or more substances (elements and/or compounds) that are not chemically combined

• Mixtures can be separated by physical methods such as filtration or evaporation

• Eg: sand and water, oil and water, sulphur powder and iron filings

  

Electron Shells

We can represent the structure of the atom in two ways: using diagrams called electron shell diagrams or by writing out a special notation called the electronicstructure

Electron shell diagrams

• Electrons orbit the nucleus in shells (or energy levels) and each shell has a different amount of energy associated with it

• The further away from the nucleus then the more energy a shell has

• Electrons occupy the shell closest to the nucleus which can hold only 2 electrons

• When a shell becomes full electrons then fill the next shell

• The second shell can hold 8 electrons and the third shell can also hold 8 electrons and the electrons organise themselves in pairs in these shells

• The outermost shell of an atom is called the valence shell and an atom is much more stable if it can manage to completely fill this shell with electrons

  

• Elements in the same group have the same number of outer shell electrons

  

%%Period%%: The red numbers at the bottom show the number of notations which is 3, showing that a chlorine atom has 3 shells of electrons

Group: The final notation, which is 7 in the example, shows that a chlorine atom has 7 outer electrons

• Noble gases= All of the noble gases are unreactive as they have full outer shells and are thus very stable

  • located 8/0

• Below is the electronic Configuration of the first 20 elements

  

The Bases of the Periodic table

• Elements are arranged on the Periodic Table in order of increasing atomic number where each element has one proton more than the element preceding it

• Hydrogen has 1 proton, helium has 2 protons, lithium has 3, etc.

• The table is arranged in vertical columns called Groupsnumbered I - VIII and in rows called Periods

• Elements in the same group have the same amount of electrons in their outer shell, which gives them similar chemicals properties

  

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Ions and ionic bonds

ions

• An ion is an electrically charged atom or group of atoms formed by the loss or gain of electrons

• An atom will lose or gain electrons to become more stable

• The loss or gain of electrons takes place to gain a full outershell of electrons which is a more stable arrangement of electrons

  

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Ionisation of metals and non-metals

• Metals: all metals can lose electrons to other atoms to become positively charged ions
• Non-metals: all non-metals can gain electrons from other atoms to become negatively charged ions

\n Electrostatic attraction

• Ionic compounds are formed when metal atoms react with non-metal atoms

• Metal atoms lose their outer electrons which the non-metal atoms gain to form positive and negative ions

• The positive and negative ions are held together by strong electrostatic forces of attraction between oppositecharges

• This force of attraction is known as an ionic bond and they hold ionic compounds together

  

This happens because formation of ionic bonds, Group 1 to VII

• Sodium is a Group I metal so will lose one outer electron to another atom to gain a full outer shell of electrons
• A positive sodium ion with the charge 1+ is formed
• Chlorine is a Group VII non-metal so will need to gain an electron to have a full outer shell of electrons
• One electron will be transferred from the outer shell of the sodium atom to the outer shell of the chlorine atom
• A chlorine atom will gain an electron to form a negatively charged chloride ion with a charge of 1-
• The oppositely charged ions are held together by strong electrostatic forces of attraction
• The ionic compound has no overall charge

^^Formula of ionic compound:^^    ^^NaCl^^

Ionic bonds happen between metals and non metals

Lattice structures: In lattice structures, the atoms are arranged in an orderedand repeating fashion

• The lattices formed by ionic compounds consist of a regular arrangement of alternating positive and negative ions

Isotopes

Isotopes are atoms of the same element that contain the same number of protonsand electrons but a different number of neutrons.

There are two types of Isotopes:

• Radioactive
• Non Radioactive

Radioactive isotopes

• Radioactive isotopes (radioisotopes) are unstable due to the imbalance of neutrons and protons, which causes the nucleus to decay over time through nuclear fission and emit radiation

  • Examples of radioisotopes include tritium and carbon-14
  • Radioactive have a lot of use in the medical field

  Example= Cancer treatments, Medical tracers, and Medical instruments and materials are routinely sterilized by exposure to radiation, which kills any bacteria present

  • the industrial uses=

  Example= Radioactive tracers are deployed in industry to detect leaks in gas or oil pipes, Geiger Counter, and Radiocarbon dating.

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Non Radioactive Isotopes

• Non-radioactive isotopes are stable atoms which really only

• isotopes share properties, why? how?

  Isotopes of the same element display the same chemical characteristics

  • This is because they have the same number of electrons in their outer shells
  • The difference between isotopes is the neutrons which are neutral particles within the nucleus and add mass only
  • The difference in mass affects the physical properties, such as density, boiling point and melting point

Metals and Non Metals

There are over 100 elements in the Periodic Table

some of them can be classified as metals and nonmetals

• Most of the elements are metals and a small number of elements display properties of both types

  • These elements are called metalloids

  

Properties of metals

• Conduct heat and electricity

• Are malleable (can be hammered and made into different shapes) and ductile (can be drawn into wires)

• Tend to be lustrous (shiny)

• Have high density and usually have high melting points

• Form positive ions through electron loss

• Form basic oxides

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Properties of nonmetal elements

• Do not conduct heat and electricity
• Are brittle when solid and easily break up
• Tend to be dull and nonreflective
• Have low density and low melting points (many are gases at room temperature)
• Form negative ions through electron gain (except for hydrogen)
• Form acidic oxides

Alloys

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• Alloys are mixtures of metals, where the metals are mixed together but are not chemically combined

• They can also be made from metals mixed with nonmetals such as carbon

• Alloys often have properties that can be very different to the metals they contain, for example they can have greater strength, hardness or resistance to corrosion or extreme temperatures

• Alloys contain atoms of different sizes, which distorts the regular arrangements of atoms

• This makes it more difficult for the layers to slide over each other, so they are usually much harder than the pure metal

  

• Metals have high melting and boiling points

  • There are many strong metallic bonds in giant metallic structures between the positive metal ion and delocalised electrons
  • A lot of heat energy is needed to break these bonds

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• Metals conduct electricity

  • There are free electrons available to move through the structure and carry charge
  • Electrons entering one end of the metal cause a delocalised electron to displace itself from the other end
  • Hence electrons can flow so electricity is conducted

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• Metals are malleable and ductile

  • Layers of positive ions can slide over one another and take up different positions
  • Metallic bonding is not disrupted as the outer electrons do not belong to any particular metal atom so the delocalised electrons will move with them
  • Metallic bonds are thus not broken and as a result metals are strong but flexible
  • They can be hammered and bent into different shapes or drawn into wires without breaking

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