3/30/2015. Third energy level. Second energy level. Energy absorbed. First energy level. Atomic nucleus. Energy released (as light)

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1 Chapter 2 An Introduction Chemistry Lecture 2: Energy Levels and Chemical Bonding Electrons are always moving Outside the nucleus in atomic orbitals Maybe usually Average distance from nucleus (size of orbital) is directly proportional to energy level Electrons in highest energy level (valence electrons) are responsible for chemical properties of the atom Energy levels of atoms are quantized Quantized: the number of possible values or states of a system is limited to certain discrete values The energies of electrons can be at certain values only, and never in between Electrons can move between orbitals When an atom becomes excited, electrons jump up in energy level Atoms are most stable in ground state Ground state: the state in which all electrons occupy the lowest energy orbital available Excited electrons will release energy as light in order to return to lower energy levels Third energy level Second energy level First energy level Atomic nucleus Energy absorbed Energy released (as light) Lowest energy level ( shell ) contains only 2 electrons 2 nd and 3 rd energy levels contain 8 electrons each Electrons at the highest energy level are on average the farthest from the nucleus These outermost electrons (valence electrons) are the ones involved in bonding 1

2 Atoms Atoms are electrically neutral Draw Configuration Diagrams H C O Hydrogen:? protons? electrons Carbon:? protons? electrons Oxygen:? protons? electrons Helium: 2 protons 2 neutrons 2 electrons Neon: 10 protons 10 neutrons 10 electrons What do these elements have in common? Ions Atoms are most stable when their valence shell is full Atoms will gain, lose, or share electrons in order to obtain a full valence shell Ions are charged particles that form when atoms gain or lose electrons Important for electrostatic attractions, electrical conduction Ions When an atom loses electrons, it has more protons than electrons This gives it what kind of charge? These are called cations Ions When an atom gains electrons, it has more electrons than protons This gives it what kind of charge? These are called anions Ionization Energy It takes energy to remove an electron from an atom Ionization energy: the minimum energy required for an electron to overcome the attractive force of its nucleus Different elements have different ionization energies The lower the ionization energy, the more likely the atom will lose an electron 2

3 Ionization Energy What do the elements with the highest ionization energies have in common? The elements with the lowest? Bonding Terminology Chemical bonds: the interaction between atoms and ions that cause them to associate with each other Ionic bonds: bonds resulting from the transfer of electrons Covalent bonds: bonds formed by the sharing of electrons Compounds: chemical made up of two or more different types of atoms or ions bonded together (Page 2-11) Electrons are transferred from one atom to another Creates cations and anions Opposites attract Product formed is called an ionic compound or a salt Individual molecules do not exist Rather, the ions arrange in a 3D crystal structure that Maximizes contact between opposite charges Minimizes contact between like charges 3

4 Electrons are shared between atoms Results in an energetically-favorable (and thus more stable) state for both atoms Results in a molecule Covalent Bonds Some molecules are made of only one type of atom (examples: oxygen, hydrogen) Most molecules are compounds Covalent Bonds By far the most common way that atoms interact Very strong require a chemical change to be broken Provide the framework for the large, complex molecules that make up the body Example: Formation of Methane Example: Formation of Water Example: Formation of Water Molecules have precise shapes Activity Complete the table on page 2-8 in your study packet Determine how many electrons the atom needs Remember: hydrogen can only form one covalent bond Atom (proton #) Symbol # of Bonds Example with hydrogen Hydrogen (1) Water looks familiar Oxygen (8) Sulfur (16) Carbon (6) Nitrogen (7) 4

5 Covalent Bonding Sometimes atoms have to share more than one pair of electrons These multiple bonds are stronger than single bonds and take more energy to break Sometimes in covalent bonds electrons are shared equally between atoms Double Bond Triple Bond Molecule of oxygen gas (O 2 ) Molecule of nitrogen gas (N 2 ) These are called non-polar covalent bonds This is not always the case What happens when you give two siblings some candy to share? The bigger stronger one will take more candy because he/she can! The same is true of bonded atoms One will likely be more electronegative Electronegativity: a measure of the attraction of an atom to a shared pair of electrons The more electronegative atom will pull more of the bonding electrons to itself This is called a polar covalent bond This asymmetry in charge density One side of the molecule is slightly positive The other side is slightly negative 5

6 Since opposites attract, positive poles on one molecule will be attracted to negative poles on another molecule These interactions are called dipole-dipole forces When a hydrogen atom is bound to a small, highly electronegative atom (usually O, N, or F) a highly polar bond is formed This results in unusually strong dipole-dipole forces called hydrogen bonds Not technically bonds intermolecular forces Weaker than covalent or ionic bonds, but strong enough to powerfully influence the properties of chemicals Best example: water Hydrogen Bonding 6

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