Periodic Table of Elements (Malvar Senior High School) PDF

PERIODIC TABLE OF ELEMENTS QUARTER 1, LESSON 3 Most Essential Learning Competencies (MELC): Differentiate among the atomic number, mass number, and isotopes, and which of these distinguishes one element from another. STEM_GC11AM-Ic-e-17 LEARNING OBJECTIVES: 1. State the periodic law...

PERIODIC TABLE OF ELEMENTS QUARTER 1, LESSON 3 Most Essential Learning Competencies (MELC): Differentiate among the atomic number, mass number, and isotopes, and which of these distinguishes one element from another. STEM_GC11AM-Ic-e-17 LEARNING OBJECTIVES: 1. State the periodic law and explain the organization of elements in the periodic table 2. Predict the general properties of elements based on their location within the periodic table 3. Identify metals, nonmetals, and metalloids by their properties and/or location on the periodic table. PHYSICAL SCIENCE PERIODIC TABLE OF ELEMENTS RAECHELLE JOYCE C. SIUDAD GENERAL CHEMISTRY 1 TEACHER PERIODIC TABLE OF ELEMENTS  As early chemists worked to purify ores and discovered more elements, they realized that various elements could be grouped together by their similar chemical behaviors. One such grouping includes lithium (Li), sodium (Na), and potassium (K): These elements all are shiny, conduct heat and electricity well, and have similar chemical properties. A second grouping includes calcium (Ca), strontium (Sr), and barium (Ba), which also are shiny, good conductors of heat and electricity, and have chemical properties in common. However, the specific properties of these two groupings are notably different from each other. For example: Li, Na, and K are much more reactive than are Ca, Sr, and Ba; Li, Na, and K form compounds with oxygen in a ratio of two of their atoms to one oxygen atom, whereas Ca, Sr, and Ba form compounds with one of their atoms to one oxygen atom. Fluorine (F), chlorine (Cl), bromine (Br), and iodine (I) also exhibit similar properties to each other, but these properties are drastically different from those of any of the elements above. Dimitri Mendeleev in Russia (1869) and Lothar Meyer in Germany (1870) Independently recognized that there was a periodic relationship among the properties of the elements known at that time. Both published tables with the elements arranged according to increasing atomic mass. Dimitri Mendeleev in Russia (1869) and Lothar Meyer in Germany (1870) Mendeleev went one step further than Meyer: He used his table to predict the existence of elements that would have the properties similar to aluminum and silicon, but were yet unknown. 31 Discoveries of gallium (1875) and germanium (1886) Ga Gallium The discoveries of these elements 69.723 provided great support for Mendeleev’s work. Although 32 Mendeleev and Meyer had a long dispute over priority, Mendeleev’s Ge Germanium contributions to the development of the periodic table are now more 72.64 widely recognized  Dimitri Mendeleev is widely credited with creating (b) the first periodic table of the elements.  By the twentieth century, it became apparent that the periodic relationship involved atomic numbers rather than atomic masses. The modern statement of this relationship, the periodic law, is as follows: the properties of the elements are periodic functions of their atomic numbers. A modern periodic table arranges the elements in increasing order of their atomic numbers and groups atoms with similar properties in the same vertical column. Elements in the periodic table are organized according to their properties.  HOW TO READ THE PERIODIC TABLE? 1 H Hydrogen 1.008 gas 1 WHAT’S IN 1 ATOMIC NUMBER THE BOX?  The atomic number refers to how many protons an atom of that element has. 1  For instance, hydrogen has 1 H Hydrogen proton, so it’s atomic number is 1.  The atomic number is unique to 1.008 that element. No two elements have the same atomic number.  2 ATOMIC MASS WHAT’S IN THE BOX?  Atomic Mass refers to the “weight” of the atom. 1  It is derived at by adding the number of protons with the H Hydrogen number of neutrons. 1.008 2 ATOMIC MASS HELIUM  This is a helium atom. Its atomic mass is 4 (protons plus neutrons). What is its atomic number? ATOMIC MASS AND ISOTOPES 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.  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.  ATOMIC MASS UNIT AMU  There are 6 X 1023 or 600,000,000,000,000,000,00 0,000 amus in one gram.  (Remember that electrons are 2000 times smaller than one amu). How do I find the number of protons, electrons, and neutrons in an element using the periodic table? Number of PROTONS = ATOMIC NUMBER Number of ELECTRONS = ATOMIC NUMBER Number of NEUTRONS = ATOMIC _ ATOMIC WEIGHT NUMBER WHAT’S IN CHEMICAL SYMBOL AND NAME THE BOX?  All elements have their own unique symbol. 1  It can consist of a single H Hydrogen capital letter, or a capital letter and one or two lower case letters. ELEMENT SYMBOL ELEMENT SYMBOL NITROGEN N POTASSIUM K SODIUM Na COPPER Cu CHLORINE Cl HYDROGEN H COMMON CARBON C HELIUM He ELEMENT COBALT Co IRON Fe AND NEON Ne NIOBIUM Nb SYMBOL GOLD Au MERCURY Hg SILVER Ag BORON B OXYGEN O FLUORINE F  VALENCE ELECTRON 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.  STATE OF MATTER AT ROOM TEMPERATURE States of Matter are the different forms that elements, compounds and mixtures will exist in as either solids, liquids or gases depending on how close their particles are. In the periodic table, the states of matter can be easily traced. All metals except for Mercury (Hg) are solids this is due to the presence of strong metallic bonding. Whilst they are all solids, some are harder than others. For example, Group 1 metals like Lithium and Sodium are soft and easy to cut. But metals such as Copper and Iron in the transition metals are strong and hard.  STATE OF MATTER AT ROOM TEMPERATURE Most non-metals are gases due to their weak intermolecular forces in their simple covalent structure. The best example of this is the top right section of the periodic table Nitrogen, Oxygen, Fluorine, Chlorine and the Noble Gases (Group 18) are all gases. As we progress down the periodic table in the non-metals however, they transition from gases to solids. With larger atoms and larger covalent structures, the likes of Sulphur, Phosphorus, Iodine and Carbon are all solids. Elements are categorized into large classes with common properties: METALS, NONMETALS, METALLOIDS  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.  PROPERTIES OF NONMETALS 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.  PROPERTIES OF METALLOIDS 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 non-metals but not as well as metals. They are ductile and malleable. The elements are arranged in seven horizontal rows, called periods or series. Elements in periods do not have similar properties  The elements are arranged in 18 vertical columns, called groups or families. Elements in families have similar properties. FAMILIES PERIODIC TABLE OF ELEMENTS PERIODIC TABLE OF ELEMENTS PERIODIC TABLE OF ELEMENTS PERIODIC TABLE OF ELEMENTS PERIODIC TABLE OF ELEMENTS PERIODIC TABLE OF ELEMENTS PERIODIC TABLE OF ELEMENTS PERIODIC TABLE OF ELEMENTS PERIODIC TABLE OF ELEMENTS PERIODIC TABLE OF ELEMENTS PERIODIC TABLE OF ELEMENTS  The elements can also be classified into the main-group elements (or representative elements) in the columns labeled 1, 2, and 13–18; the transition metals in the columns labeled 3–12; 1 and Inner transition metals in the two rows at the bottom of the table (the top- row elements are called lanthanides and the bottom-row elements are actinides  The elements can be subdivided further by more specific properties, such as the composition of the compounds they form. Hydrogen The hydrogen square sits atop Family AI, 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.  ALKALI METALS The elements in group 1 (the first column) form PERIODIC TABLE OF ELEMENTS compounds that consist of one atom of the element and one atom of hydrogen. These elements (except hydrogen) are known as alkali metals, and they all have similar chemical properties. 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.  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.  What does it mean to be 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. What does it mean to be reactive?  Alkaline Earth Metals They are never found uncombined in nature. They have two valence electrons. Alkaline earth metals include magnesium and calcium, among others.  Transition Metals Transition Elements include PERIODIC TABLE OF ELEMENTS those elements in the B 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.  Transition Metals The compounds of transition PERIODIC TABLE OF ELEMENTS 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.  Transition Elements Transition elements have PERIODIC TABLE OF ELEMENTS 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. Boron Family The Boron Family is named after the first element in the family. Atoms in this family have 3 valence electrons. This family includes a metalloid (boron), and the rest are metals. This family includes the most abundant metal in the earth’s crust (aluminum). Carbon Family Atoms of this family have 4 valence electrons. This family includes a non- metal (carbon), metalloids, and metals. The element carbon is called the “basis of life.” There is an entire branch of chemistry devoted to carbon compounds called organic chemistry. Nitrogen Family The nitrogen family is named after the element that makes up 78% of our atmosphere. This family includes non- metals, metalloids, and metals. Atoms in the nitrogen family have 5 valence electrons. They tend to share electrons when they bond. Other elements in this family are phosphorus, arsenic, antimony, and bismuth.  Oxygen Family Atoms of this family have 6 valence electrons. Most elements in this family share electrons when forming compounds. Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements.  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 non-metals. They are never found free in nature. Noble Gases A group of rare gases that include Helium, Neon, Argon, Krypton, Xenon, and sometimes Radon and that exhibit great stability and extremely low reaction rates. They all have a full outer valence shell of electrons, which makes them quite unreactive 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.