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Chapter 5

Chapter 5 . The Periodic Table. Section 5.1. In 1750, only ____ elements were known. As the rate of discovery increased, so did the _______________________the elements In 1789 _________________grouped the known elements into _______, ___________, ________, and________.

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Chapter 5

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  1. Chapter 5 The Periodic Table

  2. Section 5.1 • In 1750, only ____ elements were known. • As the rate of discovery increased, so did the _______________________the elements • In 1789 _________________grouped the known elements into _______, ___________, ________, and________.

  3. Mendeleev’s Periodic Table • Medeleev made ______________of the 63 known elements. (1863) • On each card he put the ______ of the element, _______, and ________________. • When he lined the cards up in order of increasing mass, a ___________ emerged. • Mendeleev arranged the elements into rows in order of ___________ mass so that elements with similar properties were in the _______________. A deck of cards can be divided into four suits—diamonds, spades, hearts, and clubs. In one version of solitaire, a player must produce an arrangement in which each suit is ordered from ace to king. This arrangement is a ________for Mendeleev's __________________.

  4. Periodic Table- Arrangement of elements in ________, based on a set of properties that _______ from row to row. • Mendeleev’s Prediction • He could not make ________table because many of the elements had not yet been _____________. He had to leave ________ for those elements. • Eka-Aluminum – one space below ___. He predicted it would be a ___ metal with a_____m.p. and a density of 5.9 g/cm3 • The close match between Mendeleev’s __________ and the _______ properties of new elements showed how ______ the periodic table could be. • ________ was discovered in 1875. It’s a _____ metal, m.p. is _____ ˚C, and has a density of 5.91 g/cm3 ____ from a person's hand can melt gallium. In some traffic signals, there are tiny light emitting diodes (LEDs) that contain a compound of gallium

  5. Mendeleev’s Periodic Table • How is the table organized? • Elements are arranged in order of __________ _______. • What do the long dashes represent? • They represent ______________ elements. • Why are masses listed with some of the dashes, but not with all of them? • He was able to ____________________for some unknown elements based on the properties of neighboring elements.

  6. 5.2 The Modern Periodic Table • The sounds of musical notes that are separated by an octave are ______, but they are not ________. In a similar way, elements in the ______ column of the periodic table are _______because their properties _______ at regular intervals. But elements in different rows are ____ identical.

  7. Periodic Law • Mendeleev developed his chart before the _______ was discovered. • In the modern periodic table, elements are arranged by increasing __________________. (# of _____________) • ________-Each row in the table of elements is a period. • ________-Each column on the periodic table is called a group. • Properties of elements repeat in a ___________ way when atomic numbers are used to arrange elements into groups. • Members of a group have ________ chemical properties. • This pattern of repeating properties is called ______________.

  8. Periods • Periods - the _____; represent _______ levels. • Row 1 (energy level 1) ___ elements • Row 2 and 3 (energy level 2) ___ elements • Row 4 and 5 (energy level 3) ___ elements • Row 6 and 7 (energy level 4) ___ elements • The number of available __________ increases from energy level to energy level. • Elements change from _____ to ___________ to ___________as you move from left to right across the period.

  9. Groups • Groups/Families - the _____________. • Atomic masses __________ from top to bottom. • Members of a group have similar electron ________________ and therefore have similar ____________ properties. • Tells how many valence electrons are in the last energy level of an element.*** • Valence electrons increase from _______________ on the periodic table. • ________________– an electron that is in the highest occupied energy level of an atom.

  10. Valence Electrons • A valence electron is an electron that is in the ____________________ energy level of an atom. • They play a key role in ____________________. • The # of valence electrons increases from ____ to ______. • Elements in a group have similar properties because they have the _____ __________ of valence electrons.

  11. Valence Electrons • Electron configuration is the arrangement of ____________ in an atom. • The most stable electron configuration is one in which the ___________ electron shell is completely _____________. • Atoms will ____ or ____ electrons in order to achieve the most _______ electron configuration.

  12. Atomic Mass • ______________is the # protons plus the # neutrons. • It is a value that depends on the distribution of an element’s isotopes in nature and the masses of those isotopes. • All atoms of the same element _________have the same atomic _____. • Average atomic mass of an element is a _______________of the masses of an elements isotopes. • The unit for atomic mass is –_______ • The standard on which the atomic mass unit is based is the mass of a __________________.

  13. Average Atomic Mass • _______________– some values are more important that other values • For isotopes, the one that occurs more in ______ contributes ____ to the average atomic mass.

  14. Solving for Average Atomic Mass • When solving, • Convert the % abundance to a ___________ • ________________ by its mass • ________ the products together • EX: • Chlorine-35 75.78% 0.7578 X 34.969 = 26.4995 • Chlorine-37 24.22% 0.2422 X 36.966 = +8.9532 35.4527 amu You Try:

  15. Classes of Elements • 1. Chemical symbols are ___________by solids, liquids, and gases. • The symbols for solids are _____. The symbols for liquids are _____. The symbols for gases are ____. • 2. Elements are divided into those that occur ___________ and those that do not • The symbols for elements that don’t occur naturally are ______ • 3. They are also classified by their ____________ properties. • METALS, NONMETALS, METALLOIDS • In the periodic table, metals are located on the _____, nonmetals are on the _____, and metalloids are in ____________.

  16. METALS • __________ of elements • good _____________ of heat and electricity • most are _________ at room temp. (except ___) • most are ___________ and ______ –ability to be drawn into wires • some are _________, some are not. • Ex. _____ Ex. _____ Magnesium and aluminum are typical metals

  17. Transition Metals • The metals in groups 3-12 are called __________ ________. • They form a _____ between the two sides of the table. They are well known for their ability to form compounds with _____________________ A compound of erbium (Er) and oxygen is used to tint glass pink.

  18. Nonmetals • properties are __________ of metals. • poor ____________ • many are _________ at room temp. • the solids tend to be ___________ • Some are very __________, some don’t react at all. • Ex. __is most reactive element. Ex. __ is not reactive. Toothpaste contains a compound that helps to protect teeth from tooth decay. The compound is formed from the nonmetal fluorine and the metal sodium

  19. Metalloids • elements with ___________ that fall between those of metals and nonmetals. • Ex. A metalloid’s ability to conduct electricity can vary with ___________. Si and Ge are ___________ at low temps. and _____________ at high temps. • Variation Across a Period • Across a period from left to right, the elements become _____metallic. From left to right across Period 3, there are three metals (Na, Mg, and Al), one metalloid (Si), and four nonmetals (P, S, Cl, and Ar). Many light bulbs are filled with argon gas.

  20. 5.3 Representative Groups • “___” groups are #1-8 • The number of the group is equal to the number of ______________________in an atom of that element. • Valence electrons- An electron that is in the ____________ occupied energy level of an atom.  • Elements in a group have similar properties because they have the _____________of valence electrons. • (This is why___isgrouped with metals)

  21. Alkali Metals • Group 1A • Most _________ metals • Reactivity _________ from the top to the bottom. • So reactive many are kept under ___ to prevent reacting with ______ or oxygen. • ____ Valence Electron • Found in nature only in a ______________. • Form ____ions because they will________giveup 1 electron for stability.

  22. Alkaline Earth Metals • Group 2A • Have __ Valence Electrons • ______ than the metals in 1A. • Form ___Ions because they easily give up 2 electrons for _______. • __________ used in photosynthesis within the chlorophyll. • ___________ used in teeth and bone.

  23. Boron Family • Group 3A • Have___Valenceelectrons • Form ___Ions because they easily give up 3 electrons for ____________. • 1 metalloid (________) • ___ metals • Aluminum is the most abundant metal in the Earth’s __________. • People are encouraged to ________ aluminum because it doesn’t take that much energy to do so.

  24. Carbon Family • Group 4A • Have ___ Valence Electrons • Form +/- 4 Ions because it will easily lose or gain 4 electrons for stability. (Although often doesn’t form ionic compounds) • 1 Nonmetal ________) • ___ Metalloids • ___ Metals • Metallic nature _________ from top to bottom. • With the exception of water, most of the compounds in your body contain ________. • Silicon is the second most abundant metal in the earth’s __________.

  25. Nitrogen Family • Group 5A • Have ___ Valence Electrons • Forms ___Ions because it will easily gain 3 electrons for __________. • ___ nonmetals • ___ metalloids • ___ Metals • Nitrogen and Phosphorus are used in _______________.

  26. Oxygen Family • Group 6A • Have ___ Valence Electrons • Forms ___Ions because it will easily gain 2 electrons for ____________. • ___ nonmetals • ___ metalloids • ___ metal • Oxygen is the most abundant _________ in the Earth’s _____. • _______ is another from of oxygen. At _______ level it can irritate your eyes and lungs. At higher levels it absorbs harmful radiation from the sun.

  27. Halogens • Group 7A • Have ___ Valence electrons • Form ___Ions because it will easily gain 1 electron for stability. • Most reactive ___________ increase from bottom to top. • Known as “______________” • ___ nonmetals • 1 Unknown • ___________ is the most reactive. • React easily with most __________.

  28. Noble Gases • Group 8A • ___ Valence Electrons • Helium is the ________ with only ___ valence electrons. • Extremely __________ (Do not form Ions) • _______ and __________. • Used in light bulbs. • All are used in _____ lights except argon. • Have the most ________ electron configuration.

  29. Patterns on the Periodic Table • Atomic # ________________________________. • Atomic mass ________________________. • Energy level and orbitals in rows from __________. • (Physical Properties) metals metalloids nonmetals from _____________. • Columns atomic mass from ________________. • Columns are based on chemical properties (________________). • Valence Electrons from _____________. • Most reactive metals are on the _______side. • Most reactive non-metals are on the _________ side.

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