Online Periodic Table

Transcription

1 Online Periodic Table

2 Color code the periodic table according to these guidelines: Metals -- OUTLINE whole section (NOT every individual box) in orange Nonmetals -- OUTLINE whole section in dark blue Metalloids -- OUTLINE whole section in dark green

3 The Periodic Table

4 Metals

5 Nonmetals

6 Metalloids

7 Alkali metals -- FILL IN section in red (do NOT obscure the outline color that already exists) Alkaline earth metals -- FILL IN section in yellow Halogens -- FILL IN section in light green Noble gases -- FILL IN section in light blue

8 Alkali Metals

9 Alkaline Earth Metals

10 Halogens

11 Noble Gases

12 Transition metals -- FILL IN entire section in orange Inner Transition metals -- FILL IN entire section in pink Radioactive Elements Place a black dot in the upper right corner of every radioactive element Include a legend on your periodic table explaining what each color represents.

13 Transition Metals

14 Inner Transition Metals

15 Radioactive Elements

16 chlorine nitrogen helium gold oxygen silver mercury hydrogen neodymium sodium niobium carbon

17 Elements Science has come a long way since Aristotle s theory of Air, Water, Fire, and Earth. Scientists have identified 90 naturally occurring elements, and created about 28 others.

18 Elements The elements, alone or in combinations, make up our bodies, our world, our sun, and in fact, the entire universe.

19 The most abundant element in the earth s crust is oxygen.

20 Periodic Table The periodic table organizes the elements in a particular way. A great deal of information about an element can be gathered from its position in the period table. For example, you can predict with reasonably good accuracy the physical and chemical properties of the element. You can also predict what other elements a particular element will react with chemically. Understanding the organization and plan of the periodic table will help you obtain basic information about each of the 118 known elements.

21 Key to the Periodic Table Elements are organized on the table according to their atomic number, usually found near the top of the square. The atomic number refers to how many protons an atom of that element has. For instance, hydrogen has 1 proton, so it s atomic number is 1. The atomic number is unique to that element. No two elements have the same atomic number.

22 What s in a square? Different periodic tables can include various bits of information, but usually: atomic number symbol atomic mass number of valence electrons state of matter at room temperature.

23 Atomic Number This refers to how many protons an atom of that element has. No two elements, have the same number of protons. Bohr Model of Hydrogen Atom Wave Model

24 Atomic Mass Atomic Mass refers to the weight of the atom. It is derived at by adding the number of protons with the number of neutrons. This is a helium atom. Its atomic mass is 4 H(protons plus neutrons). What is its atomic number?

25 Atomic Mass and Isotopes While most atoms have the same number of protons and neutrons, some don t. Some atoms have more or less neutrons than protons. These are called isotopes. An atomic mass number with a decimal is the total of the number of protons plus the average number of neutrons.

26 Atomic Mass Unit (AMU) The unit of measurement for an atom is an AMU. It stands for atomic mass unit. One AMU is equal to the mass of one proton.

27 Atomic Mass Unit (AMU) There are 6 X or 600,000,000,000,000, 000,000,000 amus in one gram. (Remember that electrons are 2000 times smaller than one amu).

28 Symbols C Cu Carbon Copper All elements have their own unique symbol. It can consist of a single capital letter, or a capital letter and one or two lower case letters.

29 Common Elements and Symbols

30 Valence Electrons The number of valence electrons an atom has may also appear in a square. Valence electrons are the electrons in the outer energy level of an atom. These are the electrons that are transferred or shared when atoms bond together.

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32 Properties of Metals Metals are good conductors of heat and electricity. Metals are shiny. Metals are ductile (can be stretched into thin wires). Metals are malleable (can be pounded into thin sheets). A chemical property of metal is its reaction with water which results in corrosion.

33 Properties of Non-Metals Sulfur Non-metals are poor conductors of heat and electricity. Non-metals are not ductile or malleable. Solid non-metals are brittle and break easily. They are dull. Many non-metals are gases.

34 Properties of Metalloids Silicon Metalloids (metal-like) have properties of both metals and non-metals. They are solids that can be shiny or dull. They conduct heat and electricity better than nonmetals but not as well as metals. They are ductile and malleable.

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37 Families Columns of elements are called groups or families. Elements in each family have similar but not identical properties. For example, lithium (Li), sodium (Na), potassium (K), and other members of family 1 are all soft, white, shiny metals. All elements in a family have the same number of valence electrons. Periods Each horizontal row of elements is called a period. The elements in a period are not alike in properties. In fact, the properties change greatly across even given row. The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas.

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39 Hydrogen The hydrogen square sits atop Family 1, but it is not a member of that family. Hydrogen is in a class of its own. It s a gas at room temperature. It has one proton and one electron in its one and only energy level. Hydrogen only needs 2 electrons to fill up its valence shell.

40 Alkali Metals The alkali family is found in the first column of the periodic table. Atoms of the alkali metals have a single electron in their outermost level, in other words, 1 valence electron. They are shiny, have the consistency of clay, and are easily cut with a knife.

41 Alkali Metals They are the most reactive metals. They react violently with water. Alkali metals are never found as free elements in nature. They are always bonded with another element.

42 Alkaline Earth Metals They are never found uncombined in nature. They have two valence electrons. Alkaline earth metals include magnesium and calcium, among others.

43 Transition Metals Transition Elements include those elements in the 3-12 families. These are the metals you are probably most familiar: copper, tin, zinc, iron, nickel, gold, and silver. They are good conductors of heat and electricity.

44 Transition Metals The compounds of transition metals are usually brightly colored and are often used to color paints. Transition elements have 1 or 2 valence electrons, which they lose when they form bonds with other atoms. Some transition elements can lose electrons in their next-to-outermost level.

45 Transition Elements Transition elements have properties similar to one another and to other metals, but their properties do not fit in with those of any other family. Many transition metals combine chemically with oxygen to form compounds called oxides.

46 Halogen Family The elements in this family are fluorine, chlorine, bromine, iodine, and astatine. Halogens have 7 valence electrons, which explains why they are the most active nonmetals. They are never found free in nature. Halogen atoms only need to gain 1 electron to fill their outermost energy level. They react with alkali metals to form salts.

47 Noble Gases Noble Gases are colorless gases that are extremely unreactive. One important property of the noble gases is their inactivity. They are inactive because their outermost energy level is full. Because they do not readily combine with other elements to form compounds, the noble gases are called inert. The family of noble gases includes helium, neon, argon, krypton, xenon, and radon. All the noble gases are found in small amounts in the earth's atmosphere.

48 Rare Earth Elements The thirty rare earth elements are composed of the lanthanide and actinide series. One element of the lanthanide series and most of the elements in the actinide series are called trans-uranium, which means synthetic or man-made.

49 What does it mean to be reactive? We will be describing elements according to their reactivity. Elements that are reactive bond easily with other elements to make compounds. Some elements are only found in nature bonded with other elements. What makes an element reactive? An incomplete valence electron level. All atoms (except hydrogen) want to have 8 electrons in their very outermost energy level (This is called the rule of octet.) Atoms bond until this level is complete. Atoms with few valence electrons lose them during bonding. Atoms with 6, 7, or 8 valence electrons gain electrons during bonding.

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53 Mendeleev In 1869, Dmitri Ivanovitch Mendeléev created the first accepted version of the periodic table. He grouped elements according to their atomic mass, and as he did, he found that the families had similar chemical properties. Blank spaces were left open to add the new elements he predicted would occur.

54 Matter All matter is composed of atoms and groups of atoms bonded together, called molecules. Substances that are made from one type of atom only are called pure substances. Substances that are made from more than one type of atom bonded together are called compounds. Compounds that are combined physically, but not chemically, are called mixtures.

55 Bell ringer Name a scientist that you remember and tell for what he/she is known, did, or discovered. Give any other information you can such as branch of science, prizes won, country of origin, etc.

56 Atomic Structure Defining the Atom

57 What is an Atom? The smallest part of an element that retains its identity in a chemical reaction.

58 Atomic History dkzzs

59 HISTORY OF THE ATOM 460 BC Democritus develops the idea of atoms he pounded up materials in his pestle and mortar until he had reduced them to smaller and smaller particles which could not be divided and called these: ATOMA (greek for indivisible)

60 Historic Models of the Atom Aristotle ( BC) didn t think there was a limit to the number of times matter could be divided. He knew there were small particles. Air, Fire, Earth, Water

61 HISTORY OF THE ATOM 1808 John Dalton suggested that all matter was made up of tiny spheres that were able to bounce around with perfect elasticity and called them ATOMS

62 Dalton s Atomic Theory 1. All elements are composed of atoms (which can t be divided). 2. Atoms of the same element have the same mass and atoms of different elements have different masses. 3. Compounds contain atoms of more than one element. 4. In a compound, atoms of different elements always combine in the same way.

63 Dalton s atom

64 Dalton s Atomic Theory Most of Dalton s statements are now known to be flawed. As we continue to study the atom, we will talk about discoveries that disproved Dalton s statements. Scientists have revised the theory due to new discoveries!

65 HISTORY OF THE ATOM 1898 Joseph John Thomson found that atoms could sometimes eject a far smaller negative particle which he called an ELECTRON

66 J.J. Thomson, 1897 Discovered the electron, the subatomic particle with a negative charge His experiments involved the use of a cathode ray tube Animation of Thomson s model

67 HISTORY OF THE ATOM 1904 Thomson develops the idea that an atom was made up of electrons scattered unevenly within an elastic sphere surrounded by a soup of positive charge to balance the electron's charge like plums surrounded by pudding. PLUM PUDDING MODEL

68 Thomson s Atomic Model Developed the Plum Pudding model. (think of a chocolate chip cookie) Electrons evenly distributed throughout a positively charged material.

69 Plum Pudding Model Sphere of Positive charge e- e- e- e- e-

70 HISTORY OF THE ATOM 1910 Ernest Rutherford oversaw Geiger and Marsden carrying out his famous experiment. they fired Helium nuclei at a piece of gold foil which was only a few atoms thick. they found that although most of them passed through. About 1 in 10,000 hit something

71 HISTORY OF THE ATOM helium nuclei gold foil helium nuclei They found that while most of the helium nuclei passed through the foil, a small number were deflected and, to their surprise, some helium nuclei bounced straight back.

72 Ernest Rutherford, 1911 Tested theory that electrons were evenly distributed throughout the atom within positively charged material Performed the Gold-Foil Experiment

73 Rutherford animation

74 Another Rutherford Animation

75 Ernest Rutherford If Thomson s model was correct, most of the alpha particles should pass through with a little deflection

76 Rutherford s Model Proposed that atoms contain a nucleus, a small, dense, positively-charged sphere in the center of the atom. Atom contains mostly empty space. The nucleus is tiny compared with the atom as a whole.

77 Ernest Rutherford Thomson s model Rutherford s model

78 Rutherford s model: Nuclear Atom e- e e- Rutherford did NOT know about neutrons!

79 HISTORY OF THE ATOM Rutherford s new evidence allowed him to propose a more detailed model with a central nucleus. He suggested that the positive charge was all in a central nucleus. With this holding the electrons in place by electrical attraction However, this was not the end of the story.

80 The Houston Astrodome occupies more than nine acres and seats 60,000 people. If the stadium were a model for an atom, a marble could represent its nucleus!

81 HISTORY OF THE ATOM 1913 Niels Bohr studied under Rutherford at the Victoria University in Manchester. Bohr refined Rutherford's idea by adding that the electrons were in orbits. Rather like planets orbiting the sun. With each orbit only able to contain a set number of electrons.

82 Bohr s Atom electrons in orbits nucleus

83 Summary Dalton s Theory- all matter is made up of atoms, which can t be divided Thomson s Model- discovered atoms were made up of smaller particles (these smaller particles are charged) Rutherford s Theory- discovered the positively charged nucleus

84 Development of Atomic Theory Timeline Purpose: To make an atomic theory flow map highlighting and discussing the main theories and/or discoveries for the following people or ideas: Bohr Dalton Democritus Rutherford J. J. Thomson Procedure: 1. On a piece of paper, draw a flow map consisting of five main boxes, one for each scientist listed above. 2. Place the scientists names in the correct order. (NOTE: they are listed above in alphabetical order, NOT chronological order!) Neatly write each scientist s name and the year associated with that person in the correct box. 3. Below each main box, you should add smaller boxes. Each small box should contain only one fact. Include as many boxes as necessary to highlight and discuss the main discoveries and/or theories the person is responsible for.

85 Bell Ringer What scientist expanded on the initial idea of atoms? How do we know that electrons exist?

86 Parts of an Atom Atom = nucleus surrounded by one or more electrons Atoms are neutral (no charge) same number of protons as electrons. Majority of the atom is empty space. If nucleus were the size of a pencil eraser, the closest electron would be 100 yards away! Subatomic Particles Protons (+) Neutrons (0) Electrons (-) Nucleus: Tightly packed Protons & Neutrons Electrons Orbiting speed of light!!

87 HELIUM ATOM proton Shell - + N N + - electron neutron

88 ATOMIC STRUCTURE Particle proton neutron electron Charge + charge No charge - charge Mass 1 1 nil

89 Atomic Number Atomic Number = # of Protons Each Element in the Periodic Table has a different number of Protons, therefore each element has a different, unique, atomic number. When reading the Periodic table notice each element has a unique 1 or 2 letter symbol and big & small number listed

90 ATOMIC STRUCTURE He 2 4 Atomic number the number of protons in an atom Atomic mass the number of protons and neutrons in an atom number of electrons = number of protons ***IF the atom is neutral ****

91 Can you read these?

92 Electrical Atomic Charge Remember that Atoms are neutral (no charge) So, the # of protons = # of electrons If you know the Atomic #, you know the # of Protons and also the # of Electrons!! For example: Carbon has an atomic # of 6, it therefore has 6 Protons which has an electrical charge of +6, to make the atom neutral we need 6 negative charges found in the 6 electrons orbiting the nucleus.

93 How many Neutrons are there? Remember: The Atomic # = the # of Protons The Atomic mass = The # of both Protons & Neutrons. Therefore, if you subtract the Atomic # (the number of Protons) from the Atomic mass (the number of both Protons & Neutrons) what is left over must be the number of Neutrons!! For Example w/ Carbon: Atomic Mass-Atomic # = # Neutrons Atomic Mass = 12, Atomic # = 6 Therefore there are 6 neutrons present in the Carbon nucleus If you don t believe me just count for yourself.

94 What is an Isotope? Atoms with the same number of protons, but a different number of neutrons. Same number of protons means same atomic number, which means same element. Different number of neutrons means different mass numbers.

95 Mass number (atomic mass) Atomic Mass = the total # of Protons & Neutrons ( we don t worry about the mass of the electrons since they have almost no mass)

96 Isotopes Can sometimes be represented with dashes and numbers that follow the element. C-14 Pu-246 O-16 O-17

97 Heavy Water Video clip Information about heavy water

98 Review How many protons and neutrons are there in an atom of 11 5B? A B 5 protons and 6 neutrons 5 protons and 11 neutrons C 11 protons and 5 neutrons D 11 protons and 6 neutrons

99 How many neutrons are in an element of Pu-246? A. 94 B. 150 C. 152 D. 246

100 Ions Ions are atoms that have a charge. In this case, protons do not equal electrons. Number of electrons can change based on charge of atom. Negative charge means the addition of an electron. Positive charge means you lost an electron.

101 How many protons, neutrons, and electrons? N + F -

102 Abundance of Isotopes Remember: Isotopes are atoms of the same element with different numbers of neutrons For example, the abundance of Carbon in nature may be 97% C-12, 1% C-13, and 2% C-14. This means that most of the carbon exists as C-12 and just a few atoms exist as other isotopes.

103 Average Atomic Mass You may notice that many of the atomic masses on the periodic table are in decimal numbers. This is not because these elements have partial neutrons! This is because that number is the average atomic mass of the element Average Atomic Mass

104 How to Solve for Average Atomic Mass Say you have a sample of nitrogen atoms. 95% are N-14, 1% are N-13, and 4% are N-15. You can solve for average atomic mass by multiplying by the percentages and adding the total. (.95)x14 + (.01)x13 + (.04)x15 = The average atomic mass for Nitrogen is amu.

105 You Try You have a sample of Chlorine. 50% is Cl-35, 20% is Cl-34, 20% is Cl-36, and 10% is Cl-37. What is the average atomic mass? (.50) x 35 + (.20) x 34 + (.20) x 36 + (.10) x 37= 35.2 amu

106 Beanium Lab Today you will be allowed to pick your own groups of three. You will not need goggles for this lab. You may write on the answer sheet (1 per group) I need to see 3 different handwritings for full credit. Tip: Make sure you zero the scale with your weigh boat!

107 Bell ringer 9/23/14 1. Explain Oxygen-17 and Oxygen How many protons do they each have? 3. How many neutrons do they each have?

108 Bellringer Symbol Atomic # Mass # # of Protons Hg Mo # of Electrons # of Neutrons C Pb Na Based on the number of neutrons, what can you conclude about these elements?

109 Neils Bohr, 1913 From a study of Hydrogen, concluded that an electron travels around the nucleus in circular paths called orbits Each pathway represents an energy level. Only orbits of certain energies are allowed. Electrons can t exist between orbits. Like rungs on a ladder Bohr s model animation

110 Niels Bohr Level closest to nucleus has lowest energy Energy must be added for an electron to move up a level. Energy is released when an electron moves down.

111 ATOMIC STRUCTURE Electrons are arranged in Energy Levels or Shells around the nucleus of an atom. first shell a maximum of 2 electrons second shell a maximum of 8 electrons third shell a maximum of 18 electrons

112 Bohr s Planetary Model looks like planets orbiting the sun!!! How many electrons are present in each orbit?

113 Electron Cloud Model advanced from Bohr s model Bohr s orbits are now principal energy levels. Bohr was incorrect in assuming that electrons moved like planets in a solar system. The Electron Cloud model shows the MOST LIKELY location of electrons in an atom!! (these are not precise since it s all based on probability!!) Think of a propeller on an airplane...you can see the blades when they aren t moving when it is moving you see only a blur this is like the electron cloud model!! The number of electrons in each principal energy level is still correct 2, 8, 18, 32 More atoms shown with Bohr s model

114 Which of the following provides the best analogy for an electron in an atomic orbital? a. a bee buzzing from flower to flower in a garden b. a bird flying high in the sky c. an ant crawling on the surface of a leaf d. a bee buzzing inside a closed jar

115 Quantum Mechanical Model (electron cloud model)

116 Bohr Model

117 Atomic Orbitals Orbital a region of space around the nucleus where an electron is most likely to be found (think of a map of the school and dots that mark your location every 10 minutes) Electron configuration the arrangement of electrons in the orbitals of an atom Most stable electrons are in orbitals with the lowest possible energy

118 Remember!! When electrons move to a higher orbital they GAIN energy!! When electrons move to a lower orbital they RELEASE energy!!

119 Structure of the Atom subatomic particles Proton p + Positive charge In nucleus mass =1 Neutron n o Neutral charge In nucleus mass = 1 Electron e - Negative charge In electron cloud mass = 1/1840

120 Bell Ringer Please draw electron cloud models (Bohr models) for these elements: (please make sure you show # of protons and neutrons as well!!) 1. Nitrogen 2. Argon