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Chemical Bonding

This document provides an overview of several key concepts in chemistry including: - The structure of atoms and how they interact through ionic bonds by transferring electrons or covalent bonds by sharing electrons. - How the periodic table organizes elements based on their atomic structure and valence electrons. - The formation of ions when atoms gain or lose electrons to achieve full energy levels. Ionic bonds are formed when oppositely charged ions attract. - Covalent bonds form when atoms share valence electrons to achieve full energy levels. - Polar molecules that have unequal sharing of electrons can form hydrogen bonds through weak electrostatic attractions between partially positive and negative regions.

Education◦
Atomic Interactions: Chemical Bonding Basic Chemistry i wonder why Physical Science
In your lab notebook, please answer as best you can: 1. The amount of matter in an object is its... • Mass 2. What type of property is flammability? (physical or chemical) • Chemical 3. In what state is a substance with a fixed volume but no definite shape? • Liquid 4. What does the atomic number in a Periodic Table of the Elements tell you? • The number of protons in the nucleus of that atom 4. What does the chemical formula CO2 stand for? • One carbon atom connected to two oxygen atoms, or carbon dioxide. Bonus Question: What does the atomic mass of an element tell us? Atomic mass tells how many protons plus an average of neutrons for all naturally occurring isotopes of that element. Review Quiz 2
All matter is made of atoms Atoms of the same kind are pure elements Atoms contain protons and neutrons in a central nucleus surrounded by electrons in outer energy levels. MatterMatter Interactive Periodic TableInteractive Periodic Table Review Different atoms join to form compounds When different molecules are mixed together, they either: React chemically (atoms are rearranged to form new substances) Form mixtures (intermingle but stay the same chemically)
Natural Forms of Elements • Most elements are not found in nature as pure substances. • You will never find pure sodium or chlorine gas occurring in nature. • Why is that? • Most elements are found as a combination of several different atoms joined together into compounds. • Iron is only found naturally occurring as iron ore (a mixture of iron and oxygen) • Why? Sodium Chloride CrystalsSodium Chloride Crystals Iron OreIron Ore
Van der Waals Attractions - forces between charged particles • Protons(+) ATTRACT electrons(-) • Opposite charges attract • The bigger the nucleus (more protons), the greater the attraction on electrons. • Protons(+) REPEL other protons(+) • Like charges repel • The protons of one atom will repel the protons in another atom’s nucleus Advanced Topic • Atoms that are very near each other interact because of the electrical charges of their particles. Atomic Interactions SIM
Reactivity - What makes atoms interact? • Atoms are happiest (most stable): • with full energy levels (filled electron shells) • with paired electrons • Atoms will interact with other atoms to make electron pairs and filled shells happen Phosphorus
Drawing Invisible Matter - Two ways to draw an atom • Bohr Models show ALL electrons orbiting an atom • Only valence electrons (those in the outermost shell) are involved in chemical reactions • Lewis Dot Structures display ONLY the valence electrons • Helps remove clutter & focus on just the electrons that interact Lewis StructureBohr Model Rn
Periodic Table of Elements - Bohr Diagrams
Periodic Table of Elements - Lewis Dot Structures • Elements are arranged so that atoms with the same number of valence electrons are located within the same column (group).
Ions - Unbalanced Electrons & Protons
Ions - Unbalanced Electrons & Protons • Many atoms are MUCH happier as ions (than as a neutral atom) • Cation = positive ion (remember a “cat” has “pos”) • Anion = negative ion
Ionic Bonds - TRANSFERED Electrons • Ions are formed when electrons are donated (or received) • in this case, new substances may form as ions bond together • the attraction between the opposite charges of the ions hold them together • Electrons donated/received by individual ions (charged atoms) create an IONIC BOND
Covalent Bonds - SHARED Electrons • Sometimes valence electrons are shared instead of donated • Shared electrons spend part of their time orbiting each atom's nucleus • The sharing of electrons helps keep the atoms stuck together • Electrons shared by a compound's individual atoms form a COVALENT BOND
Experiment 3.1 Milk Rainbows • Which type of milk makes the BEST rainbow? • subjective vs. objective data • Is your milk rainbow a homogeneous or heterogeneous mixture? • Are there physical or chemical changes occurring? • What interactions are happening between the molecules of milk, food coloring, and dish soap? • Observation: • What do you know? • What do you want to know? (ask a question) • Hypothesis: • Explain what you think will happen (& why) • Experiment: • Test your hypothesis • Record what happened • Conclusion: • Was your hypothesis correct? • What's next? Milk Chemistry
Hydrogen Bonds - WEAK attractions • Some covalent molecules don’t share electrons equally • O in water (H2O) has a greater pull on the shared electrons than H • Oxygen has 8 protons compared to hydrogen’s 1 • Electrons spend more time around the oxygen • The O side of the molecule then has a slightly more negative charge than the H sides • This is called a POLAR MOLECULE Advanced Topic
Molecular Polarity • Molecules that share electrons equally have no polarity (equal charge all over) • Nonpolar molecules like each other • They are all balanced • Nonpolar molecules do NOT like polar molecules (such as water) • Balanced molecules repel (push away) any slightly + or – charge • Oil (nonpolar) & water (polar) don’t mix • Detergent molecules like dish soap are both polar & nonpolar (amphipathic) • One end is polar & “loves” water • HYDROPHILIC = water loving • The slightly + and – charges flip around to fit together • The other end, a long “tail” of linked atoms, is nonpolar & “hates” water • HYDROPHOBIC = afraid of water
Metallic Bonds - Electron Soup • How many valence electrons do most metals have? • 1, 2, or 3 • These electrons are not held tightly, so they often escape • Resulting atoms are positive ions (+1, +2 or +3 charge) • Free electrons tend to float around in a constantly moving "sea" • The pooled electrons zoom around the positive ions • Give metals their unique traits • pass on heat & electricity easily (conductivity) • slide past one another easily (malleability) • commonly occur in pure metallic elements, like aluminum and copper Advanced Topic