Zusammenfassung der Ressource
CHEMICAL BONDING
- INTRAMOLECULAR
FORCES
Anmerkungen:
- Intermolecular forces are forces of attraction or repulsion which act between neighboring particles (atoms, molecules, or ions).
- Stronger than intermolecular forces
- IONIC
BONDING
Anmerkungen:
- Ionic bonding is a type of chemical bond that involves the electrostatic attraction between oppositely charged ions, and is the primary interaction occurring in ionic compounds.
- Transfer of electrons between a metal + non-metal
- PHYSICAL
PROPERTIES
- HIGH MELTING &
BOILING POINT
Anmerkungen:
- High temperatures are required to overcome the attraction between the positive and negative ions in ionic compounds. Therefore, a lot of energy is required to melt ionic compounds or cause them to boil.
- LARGE AMOUNT OF ENERGY
NEEDED TO BREAK BONDS
- HIGHER ENTHALPIES OF
FUSION & VAPORIZATION
Anmerkungen:
- They usually have enthalpies of fusion and vaporization that may be 10 to 100 times higher than those of most molecular compounds.
- The enthalpy of fusion is the heat required melt a single mole of a solid under constant pressure.
- The enthalpy of vaporization is the heat required for vaporize one mole of a liquid compound under constant pressure.
- LATTICE
STRUCTURE
Anmerkungen:
- Ionic compounds form crystal lattices rather than amorphous solids.
- HARD
Anmerkungen:
- Ionic crystals are hard because the positive and negative ions are strongly attracted to each other and difficult to separate.
- However, when pressure is applied to an ionic crystal then ions of like charge may be forced closer to each other.
- BRITTLE
Anmerkungen:
- The electrostatic repulsion can be enough to split the crystal, which is why ionic solids also are brittle.
- CONDUCTS
ELECTRICITY
- WHEN DISSOLVED IN
WATER (AQUEOUS)
Anmerkungen:
- Dissociated ions are free to conduct electric charge through the solution.
- MOLTEN STATE
Anmerkungen:
- Molten ionic compounds (molten salts) also conduct electricity.
- SOLUBLE IN
WATER (POLAR)
Anmerkungen:
- Liquids and ions are attracted to each other.
- ANION
(NON-METALS)
- ATOMS GAIN
ELECTRONS
- FORMS NEGATIVE
IONS
- CATION
(METALS)
- ATOMS LOSE
ELECTRONS
- FORMS POSITIVE
IONS
- COVALENT
BONDING
Anmerkungen:
- A covalent bond is formed between non metal atoms, which combine together by sharing electrons. .
- Covalent compounds have no free electrons and no ions so they don't conduct electricity
- POLAR COVALENT
BONDING
- UNEVEN SHARING
OF ELECTRONS
Anmerkungen:
- In a polar covalent bond, the electrons are not equally shared because one atom spends more time with the electrons than the other atom.
- PARTIAL POSITIVE AND
PARTIAL NEGATIVE ENDS
- ELECTRONEGATIVITY
VALUES MUST BE 0.4 OR
GREATER
- STRONGER INTERMOLECULAR
FORCES THAN NORMAL COVALENT
BONDS
- SIMPLE
MOLECULES
Anmerkungen:
- These contain only a few atoms held together by strong covalent bonds.
- CO2, H20, CH4, ETC.
- PROPERTIES
- LOW MELTING &
BOILING POINTS
Anmerkungen:
- Weak Van der Waals forces between molecules.
- NON-CONDUCTIVE
Anmerkungen:
- Substances with a simple molecular structure do notconduct electricity. This is because they do not have any free electrons or an overall electric charge.
- GIANT
STRCUTURES
Anmerkungen:
- Giant covalent structures contain a lot of non-metal atoms, each joined to adjacent atoms by covalent bonds.
- LATTICE
STRUCTURES
Anmerkungen:
- The atoms are usually arranged into giant regular lattices - extremely strong structures because of the many bonds involved.
- ALLOTROPES
Anmerkungen:
- Allotropes are different structural modifications of an element; the atoms of the element are bonded together in a different manner.
- GRAPHITE
Anmerkungen:
- Each carbon atom in a layer is joined to only three other carbon atoms.
- FORM
LAYERS
Anmerkungen:
- Graphite is a form of carbon in which the carbon atoms form layers. These layers can slide over each other.
- USED AS
PENCILS AND
LUBRICANT
Anmerkungen:
- The slidable layers make graphite so much softer.
- CONDUCTS
ELETRICITY
- DIAMOND
Anmerkungen:
- Diamond is a form of carbon in which each carbon atom is joined to four other carbon atoms, forming a giant covalent structure.
- VERY HARD
- HIGH MELTING
POINT
- DOESN'T CONDUCT
ELECTRICITY
- SILICA
Anmerkungen:
- Structure similar to diamond, but contains silicon and oxygen atoms, instead of carbon atoms.
- FOUND IN
SAND
- VERY HARD
- HIGH MELTING
POINT
- BUCKMINSTERFULLERENE
Anmerkungen:
- It is actually not a giant covalent structure, but a giant molecule
- FORM
HEXAGONS/PENTAGONS
- USED IN
LUBRICANTS
- METALLIC
BONDING
Anmerkungen:
- Metallic bonding is the type of bonding found in metallic elements. This is the electrostatic force of attraction between positively charged ions and delocalised outer electrons.
- ELECTRONS ARE
DELOCALIZED
- STRONG ATTRACTIVE
FORCES IN THE BOND
- PROPERTIES
Anmerkungen:
- These bonds result in physical properties of strength, malleability, ductility, and conduction.
- MALLEABLE &
DUCTILE
Anmerkungen:
- Layers of ions slide over each other.
- CONDUCTS HEAT AND
ELECTRICITY
Anmerkungen:
- There are free electrons to carry a charge.
- HIGH MELTING &
BOILING POINT
- INSOLUBLE
IN WATER
- WITHIN A
METAL
- RELATE USES OF METAL
TO PROPERTIES
- Fe
- BRIDGES/STRUCTURES
- Cu
- ELECTRICAL
WIRING
- PLUMBING
- BRASS
- COINAGE
- Al
- OVERHEAD
WIRING
- ALLOYS FOR
AIRCRAFT
- Mg
- FLARES
- HIGH STRENGTH
FOR ALLOYS FOR
AIRCRAFT
- INTERMOLECULAR
FORCES
Anmerkungen:
- An intramolecular force is any force that holds together the atoms making up a molecule or compound.
- Weaker than intramolecular forces
- HYDROGEN
BONDS
Anmerkungen:
- A hydrogen bond is a special type of dipole-dipole attraction which occurs when a hydrogen atom bonded to a strongly electronegative atom exists in the vicinity of another electronegative atom with a lone pair of electrons.
- STRONGEST
OUT OF THE 3 FORCES
Anmerkungen:
- Takes more energy to break the bonds
- IE. WATER
- COMPOSED OF 2
HYDROGENS & 1 OXYGEN
Anmerkungen:
- Because oxygen has two lone pairs, two different hydrogen bonds can be made to each oxygen
- OXYGENS SLIGHTLY
NEGATIVE
- HYDROGEN
SLIGHTLY POSITIVE
- POLAR
- ATTACHED TO ONE OF THE
MOST ELECTRONEGTIVE
ELEMENTS (N,O,F)
Anmerkungen:
- The three elements listed will grab the electrons for itself, and leave the hydrogen atom with virtually no electron density (since it had only the one).
- Now, if another molecule comes along with a lone pair, the hydrogen will try to position itself near that lone pair in order to get some electron density back.
- HYDROGEN ACQUIRE
POSITIVE CHARGE
- AT LEAST ONE
LONE PAIR
- OCCUR IN BOTH
INORGANIC AND
ORGANIC MOLECULES
- HIGH BOILING AND
MELTING POINT
Anmerkungen:
- They require more energy to break the bonds.
- PLAY A KEY ROLE IN
DETERMINING THE
PROPERTIES OF WATER
- PLAY A ROLE IN DETERMINING
THE PROPERTIES IN PROTEINS.
- VAN DER WAALS
FORCES
Anmerkungen:
- Van der Waals forces are driven by induced electrical interactions between two or more atoms or molecules that are very close to each other.
- DIPOLE-DIPOLE
FORCES
Anmerkungen:
- Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.
- HAVE POSITIVE AND
NEGATIVE REGIONS
Anmerkungen:
- Some elements have more affinity for the electrons than others, and they hang out around that atom more.
- STRONGER THAN
DISPERSION FORCES
- 5KJ - 20KJ
- POLAR
Anmerkungen:
- Slightly positive and slightly negative
- IE. ICI, SCI2,
PCI3.
- POSITIVE END ATTRACTS
NEGATIVE END
- MOLECULES NEED TO
BE VERY CLOSE
- LIKE AS IF THEY
WERE LIQUID
- TOUCHING OR ALMOST
TOUCHING
- LONDON DISPERSION
FORCES (LDF)
Anmerkungen:
- The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles.
- FOUND IN ALL MOLECULES
(POLAR&NON-POLAR)
- WEAKEST
INTERMOLECULAR FORCE
- LOWER BOILING AND
MELTING POINT
Anmerkungen:
- Bonds need less energy to break
- STRONGER BETWEEN MOLECULES
THAT ARE EASILY POLARIZED
- WEAKER BETWEEN MOLECULES THAT
ARE NOT EASILY POLARIZED