SBI4U BIOCHEMISTRY Atoms, Bonding & Molecular Polarity

Brainstorm What is a cell? What is a cell made of?

Think back… What is an atom? What is a compound? Bonus question: What is the difference between a molecule and a compound?

Atoms, Bonding, and Molecular Polarity

6 types of atoms make up 99% of all living organisms Naturally Occurring Elements in the Human Body Element Symbol Atomic # % of human body weight Oxygen O 8 65.0 Carbon C 6 18.5 Hydrogen H 1 9.5 Nitrogen N 7 3.3 Calcium Ca 20 1.5 Phosphorus P 15 1.0 Potassium K 19 0.4 Sulfur S 16 0.3 Sodium Na 11 0.2 Chlorine Cl 17 Magnesium Mg 12 0.1

Atoms and Elements Matter is any substance in the universe that has mass and occupies space All matter is composed of extremely small particles called atoms, which is the smallest unit of any given element. Every atom has the same basic structure: Subatomic Particles Core nucleus of protons and neutrons Orbiting cloud of electrons

C 6 Carbon 12.011 Atomic Number = # of protons = # electrons Symbol The element carbon - 6th element in the periodic table 6 C Carbon 12.011 Atomic Number = # of protons = # electrons Symbol Mass Number = protons + neutrons

Bohr model of a hydrogen and oxygen atom Protons Nucleus Neutrons Shells Subatomic Particles

Isotopes are atoms of the same element that vary in the number of neutrons. Nonradioactive carbon-12 Nonradioactive carbon-13 Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 7 neutrons 6 electrons 6 protons 8 neutrons Because they have the same number of protons, all isotopes of an element have the same chemical properties.

Why are electrons important? The chemical behavior of an atom is determined by its electron configuration – that is, the distribution of electrons in the atom’s electron shells. The chemical behaviour of an atom depends largely on the number of electrons in its outermost shell. (= valence electron/shell) All atoms with incomplete valence shells are chemically reactive.

C would like to N would like to O would like to H would like to Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons C would like to N would like to O would like to H would like to Gain/lose 4 electrons Gain 3 electrons Gain 2 electrons Gain 1 electron

Chemical Bonds

Atoms bond to form compounds Compounds are made up of at least 2 different kinds of atoms (e.g., H2O) Bonds are formed by the sharing or transfer of electrons Ionic Bonds 2 Types of Chemical Bonds Covalent bonds

Recall… What is the difference between an ionic bond and a covalent bond?

Opposite charges attract to form ionic bonds Ionic Bonds – occur when one atom donates or gives up one or more electrons Opposite charges attract to form ionic bonds Salt crystals Ionic Compound ( Na+Cl-)

Covalent Bonds – involve a sharing of a pair of valence electrons between atoms. Figure. 1.5, p.10

Single covalent bond Double covalent bond Four single covalent bonds Two single covalent bonds

2 Types of Covalent Bonds Polar Covalent Non-polar covalent Unequal sharing of electrons Equal sharing of electrons E.g., H2 O2 E.g., H2O Determined by the atoms ELECTRONEGATIVITY

Electronegativity the measure of the relative abilities of bonding atoms to attract electrons (Pauling Scale) In a non-polar covalent bond, there is no electronegative difference. Electrons are shared equally. E.g., O2 oxygen atoms have the same elecronegativity In a polar covalent bond, there is an electronegative difference. Electrons are shared unequally. E.g., H2O oxygen atom is more electronegative than the hydrogen atoms Electronegativity = Stronger pull of shared electrons

Polar Covalent Analogy The boy is not equally sharing with anyone else but rather taking all the food for himself.

The children are equally sharing the drink between themselves. Non-Polar Covalent Analogy The children are equally sharing the drink between themselves.

Shared electrons spend more time near the the oxygen nucleus As a result, the oxygen atom gains a slightly negative charge and the hydrogen atoms become slightly positive Water is a polar molecule because oxygen is more electronegative than hydrogen, and therefore electrons are pulled closer to oxygen.

Polar Molecules (like water) have an unequal distribution of charge. Since water is polar, it can attract other water molecules. The attraction between water molecules are called hydrogen bonds. Hydrogen bonds are weak forces between molecules

Solubility of Substances in Water Due to water’s polarity, it is a great solvent. A solvent is a substance in which a solute dissolves. A solute is what is being dissolved. What is happening in the example below? Cl- Water Na+ Na+ Water is great at dissolving both ionic (+,-) compounds and polar (partial positively, partial negatively charged molecules) molecules.

Solubility of Substances in Water: LIKE DISSOLVES LIKE! Hydrophilic (means water-loving) compounds interact with water by dissolving in it. E.g., Anions (chloride ions) in salt attracted to + poles of water Hydrophobic (means water-hating) compounds do not interact with water because they cannot form hydrogen bonds E.g., Non-polar compounds are insoluble in water Oil – non-polar compound of carbon and hydrogen

Mini-Task: Atoms, Bonding and Molecular Polarity Homework Task: Demonstrate your understanding of the relationship between electronegativity, bonding, and the polarity of molecules. *Refer to pages 9-16 in your text as well as these notes to help you conceptualize this information!

Success Criteria: Incorporate, at least, the following terms in your product: Include examples and/or diagrams where appropriate. Ensure that your product is self-explanatory (provide explanations for visual elements where appropriate) Electron(s) Atom(s) Protons Neutrons Molecules Valence shell or valence electron Covalent bond Ionic bond Cation Anion Electronegativity Non-polar covalent bond Polar covalent bond Hydrogen bond Polar molecule Reactivity or reactive Hydrophilic Hydrophobic Soluble Insoluble

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