Ions, Metals and Covalent Compounds
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- Created by: Em
- Created on: 01-06-16 07:01
Layout of the Periodic Table
- Vertical columns are called groups and horizontal rows are called periods
- Elements in groups have the same number of valence electrons as their group number (magnesium in group 2 and has 2 valence electrons)
- Elements in periods have the same number of shells (nitrogen and oxygen are both in period 2 and have 2 shells)
- The mass number of the element is the larger number and is usually rounded to 2 decimal places
- The atomic number is the smaller number and gives the number of protons (and electrons)
- The mass number is how much 1 mole (6x0.22^23) of the element is
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Isotopes
- Isotopes have the same number of protons (and electrons) but have a different number of neutrons
- They have identical chemical properties because the number of electrons/protons are the same but different physical properties (such as mass, radioactivity etc)
- Isotopes can be used for carbon dating
- Some examples of isotopes are carbon-13 and carbon-14
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Ionic bonding and Ionic Compounds
Ionic Bonding
- An ion is a charged atom, the atom is charged because it has lost or gained electrons
- Atoms lose or gain electrons to get a full valence (outer) shell
- When an atom loses an electron it becomes positive and is called a cation
- When an atom gains an electron it becomes negative and is called an anion
Ionic Compounds
- Ionic compounds have one negative and one positive ion (usually one metal and one non-metal atom)
- You can tell if an element is positive or negative by using the periodic table and looking at the group number
- The charges from the positive and negative ions have to balance out
- In solid form, ionic compounds can't conduct electricity because there aren't any free moving electrons
- However in a solution, ionic compounds can conduct electricity because the ions are free to move
- Ionic compounds have high melting and boiling points because the electromagnetic attraction is strong
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Metallic Bonding and Metal Compounds
Metallic Bonding
- Metal atoms lose electrons from their valence shell
- These lost electrons are called delocalised electrons and form a sea of delocalised electrons which is negatively charged
- This negatively charged sea of electrons are around the postive nuclei and act like a glue
- The metallic bonding is a strong, non-directional, electrostatic attraction between the positive nuclei of the atom and the delocalised electrons
Metal Compounds
- Metal compounds can conduct electricity because there is a sea of delocalised electrons so the electrical current can pass through
- They also have high melting and boiling points because the electrostatic forces between the atoms are strong so it takes more energy to break them
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Covalent Bonding and Covalent Compounds
- Covalent bonding is when non-metal atoms bond to each other by sharing an electron so they can have a full valence (outer) shell
- Covalent compounds can't conduct electricity because there are no free moving electrons or delocalised electrons
- They also have low melting and boiling points because the electrostatic attraction between the molecules is weak
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Covalent Lattices
- Covalent Lattices are non-metal atoms that are covalently conded in massive continuous structures
- These structures can be in 3D layers (diamond) or 2D layers (graphite)
- Apart from graphite, covalent lattices can't conduct electricity because there are no free moving electrons or delocalised electrons
- Covalent lattices have very high melting and boiling points because the electrostatic attraction is very strong
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Covalent Lattices
Diamond
- Diamond is made of carbon atoms that are covalently bonded to 4 other carbon atoms in a 3D structure
- A large amount of heat energy is needed to break the covalent bonds between the carbon atoms
Silica (Silicon Dioxide)
- Every silicon atom is covalently bonded to 4 oxygen atoms in a 3D structure
- Has the same properties as diamond
Graphite
- Each carbon atom is covalently bonded to other carbon atoms in a 2D structure
- There is a layer of electrons in between the layer of carbon atoms which is why graphite can conduct electricity
- This layer of electrons allows the layer of carbon to slide over each other which is why graphite is quite soft
- The covalent bonds are still strong so graphite has a high melting/boiling point
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Shapes of Molecules
- Trigonal Pyramid has 4 densities, 3 bonds and 1 lone pair
- Tetrahedral has 4 densities, 4 bonds and 0 lone pairs
- Linear has 2 densities, 2 bonds and 0 lone pairs
- Bent has 4 densities, 2 bonds and 2 lone pairs
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