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Understanding the Composition of Matter: Atoms, Elements, and Chemical Bonds

This overview explores the fundamental concepts of matter composition, including the atomic structure and the roles of protons, neutrons, and electrons. It explains how atomic numbers and mass numbers define elements while introducing the periodic table, chemical compounds, and different types of chemical bonds like ionic and covalent. The section on organic chemistry highlights the importance of carbon compounds in biological systems, summarizing key topics such as acids, bases, and the properties of water as a polar solvent.

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Understanding the Composition of Matter: Atoms, Elements, and Chemical Bonds

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  1. Composition of Matter • Atom= building block of an element • Smallest part of matter • Protons= + charge • Neutrons= 0 charge • Electrons= -1 charge

  2. Protons & neutrons= IN NUCLEUS • Electrons= Orbit OUTSIDE nucleus

  3. Subatomic Particles • Proton: positive charge, +1 mass, in nucleus • Neutron: no charge, +1 mass, in nucleus • Electron: negative charge, 0 mass, outside nucleus • ***# of protons ALWAYS = # Electrons

  4. Identifying Elements: • Atomic Number: number of protons in an element • Zr=40 protons…and _______electrons • Mass Number: Protons + neutrons • H= 1 mass # • He=4 mass #

  5. Sodium Mass Number = 23 Atomic number = 11 11 p+ 23 protons & neutrons - 11 protons ____________________ 12 n 12 neutrons In a neutral sodium atom the number of protons (11) = the number of electrons (11) 2 - 8 - 1

  6. Beryllium Mass Number = 9 Atomic number = 4 4 p+ 9 protons & neutrons - 4 protons ____________________ 5 n 5 neutrons In a neutral beryllium atom the number of protons (4) = the number of electrons (4) 2 - 2

  7. Nitrogen Mass Number = 14 Atomic number = 7 7 p+ 14 protons & neutrons - 7 protons ____________________ 7 n 7 neutrons In a neutral nitrogen atom the number of protons (7) = the number of electrons (7) 2 - 5

  8. Sulfur Mass Number = 32 Atomic number = 16 16 p+ 32 protons & neutrons - 16 protons ____________________ 16 n 16 neutrons In a neutral sulfur atom the number of protons (16) = the number of electrons (16) 2 - 8 - 6

  9. Silicon Mass Number = 28 Atomic number = 14 14 p+ 28 protons & neutrons - 14 protons ____________________ 14 n 14 neutrons In a neutral silicon atom the number of protons (14)= the number of electrons (14) 2 - 8 - 4

  10. Potassium Mass Number = 39 Atomic number = 19 19 p+ 39 protons & neutrons - 19 protons ____________________ 20 n 20 neutrons In a neutral potassium atom the number of protons (19) = the number of electrons (19) 2 - 8 - 8- 1

  11. Periodic Table • Columns on the table are called Groups • Group # is # of valence electrons • Rows are called Periods • Period # tells how many shells you have

  12. Atomic Weight & Isotopes • Isotopes= same # of protons & electrons, but DIFFER in neutrons • Ex) Hydrogen, H2, H3 • They still have same chemical properties • Radioisotopes= heavier isotopes that are unstable and decay • Can be harmful to cells • Can be used to tag biological molecules

  13. Chemical Compounds • Chemical combination of 2 or more elements • Water = H2O • A compound can behave differently than the elements that make it up • Ex) Water. Hydrogen is gas, Oxygen is gas. Together they form a liquid.

  14. Types of Chemical Bonds: • Ionic Bond: when electrons are transferred from one element to another • When an atom gains electrons, it becomes negatively charged and is called Anion. • Cation = positive charge, when element gave up electron

  15. Covalent Bonds: • When atoms share electrons • The valence shell is satisfied by both molecules

  16. Van der Waals Forces • When atoms share electrons, sharing is not always equal. • + and – charges attract to each other

  17. Water Polarity • Because of unequal distribution of electrons, water is polar. • Negative pole of oxygen is attracted to the positive pole of hydrogen

  18. Solutions & Suspensions • Solutions=all components in a mixture are equally distributed • Suspensions= mixture of water and undissolved solutes • Solute=substance dissolved • Solvent=dissolves solute

  19. Acids and Bases • Acids=produces H ions • Value below 7 • Bases=produce OH ions • Value above 7 • Look on pg. 43

  20. pH Scale • Created to indicate the concentration of H ions. • Low # = acid • High #= base

  21. Carbon Compounds • Organic Chemistry is the study of all compounds containing carbon • Carbon can form millions of different bonds • 4 types of compounds: • Carbs Nucleic acids • Lipids Proteins

  22. Carbs= main source of energy • Proteins= form bones, muscles, made of amino acids • Nucleic Acids= store/transmit genetic information • Lipids= store energy, make up membranes

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