Periodic Table of Elements PDF

1 3 H Li 11 Na PERIODIC TABLE OF ELEMENTS 4 Be 19 12 K Mg 37 19 Rb Ca ...

1 3 H Li 11 Na PERIODIC TABLE OF ELEMENTS 4 Be 19 12 K Mg 37 19 Rb Ca  A chemical element is a pure BASICS substance that consists of one type of atom. Each atom has an atomic number, which represents GROUP 1 the number of protons that are Elements in the nucleus of a single atom of that element. The periodic table of elements is ordered by GROUP 2 ascending atomic number. The chemical elements are divided G OUPS R into the metals, the metalloids, and 3-12 the nonmetals. Metals, typically found on the left side of the GROUP 17 periodic table, are: - often conductive to electricity GROUP 18 - malleable - shiny SLIDESMANIA.COM - sometimes magnetic La & Ac Series 2  History of the Periodic Table Antoine Lavoisier (1743 – 1794) – Published Elements of Chemistry in 1789 Included a list of “simple substances” (which we now know to be elements) Formed the basis for the modern list of elements – Only classified substances as metals or nonmetals The earliest attempt to classify elements was grouping the then known elements (about 30 elements) into two groups called metals and non metals. SLIDESMANIA.COM  Johann Döbereiner (1780 – 1849) – Classified elements into “triads” Groups of three elements with related properties and weights Began in 1817 when he realized Sr was halfway between the weights of Ca and Ba and they all possessed similar traits – Döbereiner’s triads: Cl, Br, I S, Se, Te Ca, Sr, Ba Li, Na, K SLIDESMANIA.COM  John Newlands (1837 – 1898) – Law of Octaves (1863) Stated that elements repeated their chemical properties every eighth element Similar to the idea of octaves in music SLIDESMANIA.COM  Dmitri Mendeleev (1834 – 1907) – Russian chemist (“The father of the periodic table”) – Arranged elements based on accepted atomic masses and properties that he observed – Listed elements with similar characteristics in the same family/group SLIDESMANIA.COM  b) Mendeleev’s periodic table - Mendeleev classified elements in the increasing order of their atomic masses and similarities in their properties. - Mendeleev’s periodic table has 6 horizontal rows called periods and 8 vertical rows called groups. The groups 1 to 7 had two sub groups called A sub group and B sub group. Group 8 had 3 rows of elements. Elements having similar properties were placed in the same groups. There are some spaces left vacant in the table to accommodate the elements to be discovered in future. Merits of Mendeleev’s periodic table :- i) Elements were classified on a more fundamental basis of their atomic masses and properties. ii) Spaces were left vacant to accommodate the elements to be discovered in future. iii) It could predict the properties of the elements which helped in the discovery of new elements. iv) The inert gas elements discovered later could be placed in a separate group without disturbing the table.  Henry Moseley (1887 – 1915) – English physicist – Arranged elements based on increasing atomic number Remember: atomic number = # of p+ in nucleus – Periodic table looked similar to Mendeleev’s design since as atomic number increases, so does the atomic mass SLIDESMANIA.COM  Vertical Columns: BASICS Horizontal Rows: ❖ The vertical columns on the periodic table are ❖ The horizontal rows on the periodic table are GROUP 1 called groups called periods ❖ Elements in the same group have very similar ❖ Elements in the same period all have the same properties GROUP 2 number of electron orbitals ❖ Groups all have the same number of valence ❖ There are 7 periods on the periodic table electrons GROUPS 3-12 ❖ There are 18 groups on the table GROUP 17 GROUP 18 SLIDESMANIA.COM La & Ac Series 9  MAJOR 1 3 H Li CLASSES OF 11 Na ELEMENTS Metals, Metalloids, and 4 Be 19 12 K Mg Nonmetals. 37 Rb 19 Ca  Helpful terms to know: BASICS Metals ❖ Conductivity: a material’s ability to conduct (transfer) electricity or heat GROUP 1 Metals are substance with high electrical ❖ Malleability: the ability of a metal to be conductivity, luster, and malleability, which readily hammered into thin sheets (gold and silver are loses electrons to form positive ions (cations). highly malleable) or the quality of something GROUP 2 that can be shaped into something else The majority of the periodic table is composed of without breaking. elements that are metals at room temperature. GROUPS 3-12 Metals The METALS are pink on the periodic table below Physical State Solid at room temp. (except Hg) GROUP 17 Appearance Shiny/lustrous Conductivity Good conductor GROUP 18 Malleability Good Melting Point Generally High SLIDESMANIA.COM La & Ac Boiling Point Generally High Series 11  Helpful terms to know: BASICS Nonmetals ❖ Conductivity: a material’s ability to conduct (transfer) electricity or heat Nonmetals are those which lack all the metallic GROUP 1 ❖ Malleability: the ability of a metal to be attributes. They are good insulators of heat and hammered into thin sheets (gold and silver are electricity. highly malleable) GROUP 2 Nonmetals are found on the right side of the periodic table, with the exception of hydrogen. Nonmetals GROUPS 3-12 The NONMETALS are blue on the periodic table below. Physical State Solid, Liquid, Gas (majority) Appearance Non-shiny GROUP 17 Conductivity Poor conductor Malleability Poor GROUP 18 Melting Point Generally Low SLIDESMANIA.COM Boiling Point Generally Low La & Ac Series 12  METALLOIDS The list of metalloids elements are: BASICS - Boron (B) - Silicon (Si) Metalloids can be defined as chemical elements - Germanium (Ge) - Arsenic (As) GROUP 1 whose physical and chemical properties fall in between the metal and non-metal categories - Antimony (Sb) - Tellurium (Te) - Astatine (At) Most periodic tables will have a dark line zig zagging GROUP 2 between the metals and nonmetals. This is called Metalloids the “stair stepper” Physical State Generally solid GROUPS 3-12 The METALLOIDS are orange on the periodic table below and are found on either side of the stair Appearance Shiny stepper. Conductivity Semiconductor GROUP 17 Malleability Brittle Melting Point Medium GROUP 18 Boiling Point Medium SLIDESMANIA.COM ❔ What do you notice about the properties of metalloids La & Ac Series when compared to metals and nonmetals? 13  BASICS Alkali Metal GROUP 1 Alkali metals belong to the s-block elements occupying the leftmost side of the periodic table. Alkali metals readily lose electrons, making them GROUP 2 count among the most reactive elements on earth. - they react with water, they usually form GROUPS 3-12 alkalies which are nothing but strong bases that can easily neutralise acids. Alkali Metals Physical State Solid GROUP 17 Appearance Shiny/lustrous Conductivity Good conductor GROUP 18 Malleability Good SLIDESMANIA.COM Melting Point low La & Ac Series Boiling Point low 14  BASICS GROUP 1 ALKALI METALS ❖ Group 1 metals all have one valence electron GROUP 2 ❖ They like to give this electron away so their outer orbitals are full GROUPS 3-12 ❖ This group is the most reactive on the periodic table The video above demonstrates 3 alkali metals GROUP 17 reacting with water. The water in the beaker contains phenolphthalein which is an indicator. Phenolphthalein is clear in acidic conditions (pH < GROUP 18 7) and turns pink in basic conditions (pH > 7) SLIDESMANIA.COM La & Ac Series 15  BASICS ALKALI METALS Due to their high reactivity, alkali metals do not occur naturally in their pure form - they are often bonded to another element, forming a compound. GROUP 1 ALKALI METALS These metals are so reactive that, in their pure So what happened in those beakers? form, they must be stored in mineral oil to prevent GROUP 2 them from readily reacting with the air. 🧪 The alkali metals reacts violently with water GROUPS 3-12 🧪 This produced lithium hydroxide, sodium hydroxide, and potassium hydroxide (this compound is what caused the indicator to GROUP 17 turn pink) 🧪 Hydrogen gas was also produced along with a lot of heat GROUP 18 🧪 The exothermic conditions of this reaction caused the hydrogen gas to catch fire SLIDESMANIA.COM La & Ac Series 16  BASICS The metals in Group II of the periodic table are Alkaline Earth Metal called the alkaline earth metals. They are: - beryllium (Be) - magnesium (Mg) GROUP 1 Alkali metals The name “alkaline” comes from the - calcium (Ca) fact that compounds of these elements form basic - strontium (Sr) - barium (Ba) (pH greater than 7) or alkaline solutions when - radium (Ra) GROUP 2 dissolved in water. - alkaline earth metals are the second most GROUPS 3-12 reactive family of elements Alkaline Earth Metals Physical State solid GROUP 17 Appearance Shiny/lustrous Conductivity Good conductor GROUP 18 Malleability Good SLIDESMANIA.COM Melting Point low La & Ac Series Boiling Point low 17  BASICS GROUP 2 Fun Fact: The alkaline earths get their names from their GROUP 1 oxides, which were known to humankind long before ALKALINE EARTH METALS the pure elements were isolated. These oxides were Group 2 elements have two valence electrons and called beryllia, magnesia, lime, strontia, and baryta. GROUP 2 like to give them away so their outer orbitals are full The word "earth" in this use comes from an old term used by chemists to describe a nonmetallic These metals are soft and silver but have less substance that did not dissolve in water and GROUPS 3-12 metallic character than the Group 1 metals resisted heating. It wasn't until 1780 that Antoine Lavoisier suggested the earths were compounds With the exception of beryllium, Group 2 metals rather than elements. Source readily react with water. GROUP 17 GROUP 18 SLIDESMANIA.COM La & Ac Series 18  BASICS Transition Metal Transition metals any of various metallic elements GROUP 1 (such as chromium, iron, and nickel) that have valence electrons in two shells instead of only one. GROUP 2 -These metals are versatile in use like iron is used in Transition Metals manufacturing and construction, and titanium is Physical State Solid at room temp. (except Hg) used in the medical field for artificial hip GROUPS 3-12 replacements. Appearance Shiny/metallic Conductivity Good conductor GROUP 17 Malleability Good Melting Point high GROUP 18 Boiling Point high SLIDESMANIA.COM La & Ac Series 19  BASICS TRANSITION METALS GROUP 1 TRANSITION METALS Groups 3 through 12 on the periodic table are the GROUP 2 transition metals. The name “transition metals” originates from two GROUPS 3-12 main ideas. The transition metals are also named so because of what is happening with their valence electrons. The elements in Groups 3 through 12 act as a bridge GROUP 17 between the highly metallic alkali and alkaline earth Most elements use the electrons from their metals on the left to the nonmetals on the right. outermost orbital to bond with other elements. These elements help transition between the metals GROUP 18 and nonmetals. Transition metals are able to use two of their outermost orbitals to bond with other elements. The transition metals have two orbitals that are not SLIDESMANIA.COM “happy” so both orbitals are able to bond with other La & Ac Series elements. 20  METALLOIDS The list of metalloids elements are: BASICS - Boron (B) - Silicon (Si) Metalloids can be defined as chemical elements - Germanium (Ge) - Arsenic (As) GROUP 1 whose physical and chemical properties fall in between the metal and non-metal categories - Antimony (Sb) - Tellurium (Te) - Astatine (At) Most periodic tables will have a dark line zig zagging GROUP 2 between the metals and nonmetals. This is called Metalloids the “stair stepper” Physical State Generally solid GROUPS 3-12 The METALLOIDS are blue on the periodic table below and are found on either side of the stair Appearance metallic stepper. Conductivity Semiconductor GROUP 17 Malleability Brittle Melting Point Medium GROUP 18 Boiling Point Medium SLIDESMANIA.COM ❔ What do you notice about the properties of metalloids La & Ac Series when compared to metals and nonmetals? 21  The following are the general properties of non-metals: BASICS Non-Metal - The atoms of non-metals tend to be smaller than those of metals. Several of the other properties of non-metals result from their atomic sizes. GROUP 1 Non- metals - are those which lack all the metallic - Non-metals have high electronegativities. This means attributes. They are good insulators of heat and that the atoms of non-metals have a strong tendency to attract more electrons than what they would normally electricity. They are mostly gases and sometimes have. GROUP 2 liquid. Some of then are even solid at room - In contrast, metals rather easily give up one or more temperature like Carbon, sulphur and phosphorus. electrons to non-metals, metal therefore easily form positively charged ions, and metals readily conduct electricity. GROUPS 3-12 Non- Metals Physical State gas GROUP 17 Appearance Shiny/lustrous Conductivity Good conductor GROUP 18 Malleability Good SLIDESMANIA.COM Melting Point low La & Ac Series Boiling Point low 22  BASICS Halogens The group of halogens is the only periodic table group that contains elements in all three familiar states of matter at standard temperature and pressure Halogens - Halogens are nonmetals. At room GROUP 1 - Fluorine (F) is a pale yellow gas temperature, fluorine and chlorine are gases, - Chlorine (Cl) is a greenish gas bromine is a liquid and Iodine and astatine are - Bromine (Br) is a dark red liquid solids. Halogens are very reactive, the reactivity - Iodine (I) is a black solid, and when heated, it GROUP 2 forms a purple vapour decreases from fluorine to astatine. Halogens do not - Astatine (At) is a black solid exist in elemental form in nature. Astatine isotopes The halogens have a strong and often nasty GROUPS 3-12 are radioactive with short half-lives. smell The halogen elements are extremely toxic Alkali Metals GROUP 17 Physical State solid, liquid and gas Conductivity poor conductor GROUP 18 Malleability poor SLIDESMANIA.COM Melting Point low La & Ac Series Boiling Point low 23  BASICS HALOGENS GROUP 1 HALOGENS The halogens are highly reactive because they have GROUP 2 7 valence electrons and only need 1 more to fulfill the outermost orbital. GROUPS 3-12 Halogens readily bond with alkali metals - they’re the perfect match: GROUP 17 ⚛ Alkali metals have one valence electron they want to give away ⚛ Halogens desperately want to gain one more GROUP 18 electron SLIDESMANIA.COM La & Ac Series 24  BASICS Halogens are never found in their pure form in Page 2 nature — they are too reactive. Instead, halogens in their “pure” form are diatomic GROUP 1 molecules: F2 Cl2 Br2 I2 A diatomic molecule is one that is made up of two GROUP 2 atoms. Most diatomic molecules are of the same element though a few combine different elements GROUPS 3-12 GROUP 17 GROUP 18 The above video demonstrates the reactivity of the halogens. SLIDESMANIA.COM La & Ac Series 25  - The Noble gases were not discovered until 1892 BASICS Noble Gas because the noble gases are highly unreactive, they remained hidden in the atmosphere. They make up Noble gases are located in Group 18 (VIIIa) of the only 1% percent of the atmosphere. GROUP 1 periodic table. Also known as the inert gases. Noble gas is translated from the German noun Edelgas, first used in 1898 by Hugo Erdmann to indicate their The noble gases: are helium (He), neon (Ne), GROUP 2 extremely low level of reactivity. argon (Ar), krypton (Kr), xenon (Xe), radon (Rn), and ununoctium (Uuo). - The name makes an analogy to the term "noble GROUPS 3-12 metals", which also have low reactivity. Noble Gas Physical State Gas GROUP 17 Appearance colorless, odorless,tasteless Conductivity Very poor conductor GROUP 18 Malleability poor SLIDESMANIA.COM Melting Point very low La & Ac Series Boiling Point very low 26  BASICS NOBLE GASES GROUP 1 NOBLE GASES Group 18 elements are called the noble gases. GROUP 2 These elements are the most stable on the periodic table because they naturally have a full outer orbital GROUPS 3-12 of electrons. Due to their full outer orbital of electrons, the noble GROUP 17 gases rarely react with other elements. GROUP 18 SLIDESMANIA.COM La & Ac Series 27  Lanthanides are the rare earth elements of the modern periodic BASICS Lanthanide table. - They are called rare earth metals since the occurrence of these elements is very small (3×10-4 % of the Earth’s GROUP 1 Alkali metals bs. crust). - The term ‘lanthanide’ was first introduced by the Norwegian mineralogist Victor Goldschmidt in the year - The lanthanide (or lanthanoid or lanthanoid) 1925. series of elements consists of fifteen metallic GROUP 2 - The lanthanide family consists of fifteen metallic chemical elements, which, along with elements scandium and yttrium, are known as the rare GROUPS 3-12 earth elements. Lanthanide Physical State solid at room temperature. lustre and are silvery in GROUP 17 Appearance appearance. Conductivity Good conductor GROUP 18 Malleability Good SLIDESMANIA.COM Melting Point very high La & Ac Series Boiling Point very high 28  BASICS Actinide All actinide series elements are radioactive in nature, they release a large amount of GROUP 1 Actinide - The term ‘actinide series’ has been energy on radioactive decay. Uranium and derived from the first element of the series, thorium are the most abundant naturally actinium. The symbol An is used to refer to any of occurring actinides on earth, whereas GROUP 2 the actinide series elements, which range in the plutonium is synthetically obtained. periodic table from atomic numbers 89 to 103. GROUPS 3-12 Actinide Physical State solid GROUP 17 Appearance silvery/lustrous Conductivity Good conductor GROUP 18 Malleability Good SLIDESMANIA.COM Melting Point high La & Ac Series Boiling Point high 29  BASICS LANTHANIDE & ACTINIDE SERIES These two rows of elements are called the LANTHANIDE SERIES (elements 57-71) and the ACTINIDE SERIES (elements 89-103). GROUP 1 Look at the atomic numbers of the elements at the bottom of the periodic table. Where does this These rows are also called the “inner transition rectangle of technically elements belong on the metals” GROUP 2 table? Lanthanides are all metals and are similar to the reactivity of Group 2 metals. GROUPS 3-12 ⚛ Lanthanides are used in optical devices (night vision goggles), petroleum refining, GROUP 17 and alloys Actinides are all radioactive elements GROUP 18 ⚛ Actinides are used in applications where their radioactivity can be used to power SLIDESMANIA.COM devices (e.g., cardiac pacemakers) La & Ac Series 30 Periodic Properties & Trends Electronegativity – Ability of an atom to pull e- towards itself – Increases going up and to the right Across a period 🡪 more protons in nucleus = more positive charge to pull electrons closer Down a group 🡪 more electrons to hold onto = element can’t pull e- as closely Periodic Properties & Trends Atomic Radius – Distance between the nucleus and the furthest electron in the valence shell – Increases going down and to the left Down a group 🡪 more e- = larger radius Across a period 🡪 elements on the right can pull e- closer to the nucleus (more electronegative) = smaller radius *Remember* – LLLL 🡪 Lower, Left, Large, Loose Periodic Properties & Trends Ionization Energy – Energy required to remove an e- from the ground state – 1st I.E. = removing 1 e-, easiest – 2nd I.E. = removing 2 e-, more difficult – 3rd I.E. = removing 3 e-, even more difficult Ex.) B --> B+ + e- I.E. = 801 kJ/mol Ex.) B+ --> B+2 + e- I.E.2 = 2427 kJ/mol Ex.) B+2 --> B+3 + e- I.E.3 = 3660 kJ/mol Periodic Properties & Trends Ionization Energy Increases going up and to the right – Down a group 🡪 more e- for the nucleus to keep track of = easier to rip an e- off – Across a period 🡪 elements on the right can hold electrons closer (more electronegative) = harder to rip an e- off Periodic Properties & Trends Metallic Character – How “metal-like” an element is Metals lose e- – Most Metallic: Cs, Fr – Least: F, O – Increases going down and to the left Think about where the metals & nonmetals are located on the periodic table to help you remember! Periodic Properties & Trends Ionic Radius – Radius of an atom when e- are lost or gained🡪 different from atomic radius – Ionic Radius of Cations Decreases when e- are removed – Ionic Radius of Anions Increases when e- are added Overall Periodic Trends Property Group Trend Period Trend Increases going down Increases to the left Atomic Radius Increases going up Increases to the right Ionization Energy Increases going up Increases to the right Electronegativity Increases going down Increases to the left Metallic Character Summary of Trends: Check your understanding: electronegativity electronegativity