Leaving Cert Chemistry. Free Notes. Chemical Bonding
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1 Leaving Cert Chemistry Free Notes Chemical Bonding
2 Chemical Bonding: Molecule: Group of atoms which are chemically joined e.g. 2 0, CO 2 and C 4. A molecule can be polar or non polar. Difference between polar and non polar atoms Polar Non polar Atoms in the molecule have slight charges Atoms in the molecule have no charges because they share a pair of electrons because they share a pair of electrons equally unequally e.g. δ+ Cl δ- e.g. - Covalent bond: This is the bond formed when two or more atoms attract a shared pair of electrons Electronegativity: This is the measure of the tendency of an atom to attract a shared pair of electrons in a covalent bond. Note: Every atom is given an EN value found in a table. Small non metal atoms are better at attracting a shared pair rather than a large metal one. The most electro negative attracting element is fluorine. EN values vary going across a period of elements: The EN values increase going across the period of elements This means the small non metal atoms on the RS are better at attracting shared pair of electrons. Reasons: Nuclear charge increases 1) The number of protons or positive charges in the nucleus increases. 2) The atomic radius decreases. The smaller atomic radius means that the shared pair will be closer to the increasing nuclear charge. EN values change going down a group: EN values decrease, Reasons: The atomic radius increases. The nuclear charge increases, BUT its affect is screened by an extra shell of electrons. Page 2 of 5
3 Li 3 2, 1, Na 11-2, 8, 1 K 19 2, 8, 8, 1 Use of EN values in chemistry: EN values are used to predict the type of bond which forms between atoms. ow? E. N. Equal to or > 1.7 = ionic bond E. N. > 0.4 but < 1.7 = polar covalent (share pair of electrons unequally) E.N. = 0 to 0.4 pure covalent bond (share pair of electrons equally) Q) What is the difference between a pure covalent bond and a polar covalent bond? Pure Covalent Polar Covalent Bond formed between two atoms when they Bond formed between two atoms when they share a pair of electrons equally. EN = 0 share a pair of electrons unequally e.g., Cl Cl e.g. 2 0 Note: Linus Pauling measured the electronegativity of each element and put them in a table. If you read various books or sources the Noble gases are not in this table because they do not form bonds. Dative covalent bond: Bond formed between two atoms when they share a pair of electrons but the shared pair comes from one of the atoms. Polarity: To show if a compound [usually a liquid] is polar, pour the liquid from a burette past a charged rod, for example rub a pen vigorously on a woollen cloth. If the liquid is not polar it will pass the rod un-deflected The stream will be deflected if it is polar If the charge of the rod is reversed the stream still bends opposite end of molecule is attracted Bond formation Q) Using a dot and cross diagram to show the bonding in an ammonia, N 3, molecule. (2009, l, 7 marks) Join N with three atoms. N (group 5) > valency of 3 i.e. needs 3 electrons from other atom(s) for it to become stable. (group 1) > valency of 1 i.e. needs one more electron to be stable. NOTE TE RELEVANCE OF VALANCY IN FUTURE Page 3 of 5
4 N 3 Ammonia N has an Atomic Number of 7 and 7 electrons in ground state Electron pattern 2,5 N Lone Pair N has 5 e- on outer shell 3 of these 5 are involved in bonding The N3 has a pyramidal shape. Bonding Pairs Q) Write the chemical formula for hydrogen sulphide. Use clear cross and dot diagrams to show the binding in ydrogen sulphide. Would you expect hydrogen sulphide molecule to be linear or non linear? Justify your answer Formula: 2 S S with two hydrogen atoms S (group 6) > valency of 2 S has 6 electrons in its outer shell, 2 of these are involved in bonding. Molecule with two lone pairs. As a result it is V shape Therefore it is non linear Valance shell electron pair repulsion theory (VSEPR)? 1) This is a theory used in chemistry to predict the shape which molecules have. Main points of theory: The shape of a molecule depends on the: 1) Number of electron pairs around a central atom and 2) The type of these electron pairs i.e. lone pairs and bond pairs. The different pairs of electrons repel each other and try to be as far as possible away from each other. Page 4 of 5
5 The strongest repulsion is between the two lone pairs with the weakest are between two bond pairs. The presence of a lone pair on the central atom: a) Forces bond pairs closer together b) Reduces the bond angle Results: 1) 4 bond pairs (around central atom) tetrahedral shape e.g. C 4 (methane) Tetrahedral Bond Angle C = Methane C 4 C 4 bonding pairs All repel equally Move as far apart as possible Bonding Pairs Note they are NOT on the equator but one at the pole and three below the equator For more comprehensive Leaving Cert Chemistry Revision Notes Click ere. Leaving Cert Chemistry Notes Page 5 of 5
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