Element # of protons # of neutrons # of electrons Carbon (atomic # 6) Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Oxygen (atomic # 8) Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Hydrogen (atomic # 1) Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Nitrogen (atomic # 7) Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: How does the number of electrons affect how many bonds are formed by these atoms? Define the following (see boxes on pp 31, 33) Polar covalent bond Non-polar covalent bond Ionic bond Hydrogen bond Hydrophobic Hydrophilic Amphipathic Element # of protons # of neutrons # of electrons Carbon (atomic # 6) Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Oxygen (atomic # 8) Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Hydrogen (atomic # 1) Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Nitrogen (atomic # 7) Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Neutral atom: Ion: Isotope: Solution Element # of protons # of electrons # of neutrons Ion Isotopes Carbon 6 6 6 C+4 or C-4 Carbon-12 which has 6 protons and 6 neutrons and 6 electrons. Carbon-14 which has 6 protons, 8 neutrons and 6 electrons. Oxygen 8 8 8 Oxygen generally forms O-2. It has 6 electrons in the outermost orbit. Three stable isotopes of oxygen are found- O-16,O17 and O-18. Hydrogen 1 1 1 Hydrogen has a charge of +1. Hydrogen has 3 stable isotopes – protium (1 proton and 1 electron), deuterium (1 proton, 1 electron and 1 neutron) and tritium (1 proton, 1 electron and 2 neutrons) Nitrogen 7 7 7 Usually has the charge -3. N-14 has odd number of protons and neutrons (7 each). N-15 has protons and 8 neutrons. Carbon does not usually form an ion by loss or gain of 4 electrons. It shares its 4 electrons with 4 others to complete its orbit and forms a covalent bond. Oxygen has 6 valence lectrons in its outermost shell, therefore it can form 2 bonds Hydrogen atom has one valence electron in its outermost orbit. The maximum capacity of its orbital is 2 electrons. Nonpolar covalent bond Non-polar covalent bond is formed when the atoms (with similar electron affinity) share electrons equally. The electronegativity difference between the two bonded atoms is usually less than 0.5. Examples – diatomic molecules H2 and N2. Polar covalent bond Polar covalent bond is formed when the electrons are not equally shared i.e. the atom with higher electronegativity (affinity) pulls the electrons towards itself. The compound which is formed has electrostatic potential and has the ability to form weak bonds with other polar molecules. The electronegativity difference between bonded atoms is 0.5 to 1.9. Examples include water, ozone. Ionic bond – the valence electrons are completely transferred from one atom to another. The metal lo.