Periodic Table of Elements

PERIODIC TABLE OF ELEMENTS PREPARED BY: MS. ANN KIMBERLY S. MENDOZA  HISTORY OF THE PERIODIC TABLE JOHANN W. DOBEREINER (1871) Law of Triads – Elements with similar properties were arranged in groups of three. Ex. Chlorine, Bromine, Iodine, Iron, Cobalt, and Nickel JOH...

PERIODIC TABLE OF ELEMENTS PREPARED BY: MS. ANN KIMBERLY S. MENDOZA  HISTORY OF THE PERIODIC TABLE JOHANN W. DOBEREINER (1871) Law of Triads – Elements with similar properties were arranged in groups of three. Ex. Chlorine, Bromine, Iodine, Iron, Cobalt, and Nickel JOHN NEWLAND Law of Octaves - There is a repetition of similar properties for every eighth element. Ex. Fluorine and chlorine, lithium and sodium JULIUS LOTHAR MEYER developed a periodic table with 56 elements, grouped according to their valence and properties. PREPARED BY: MS. ANN KIMBERLY S. MENDOZA DMITRI MENDELEEV Known as the “Father of the Modern Periodic Table“; he published a table of elements and arranged elements in order of increasing atomic weight. The elements in Mendeleev’s table are arranged in rows called periods and vertical columns called groups. He placed the elements with similar properties in the same group. Henry G. Moseley determined the atomic number and arranged the elements in order of increasing atomic numbers. He proposed the modern periodic law, which states that the chemical and physical properties of elements are the periodic function of their atomic numbers. PREPARED BY: MS. ANN KIMBERLY S. MENDOZA  ELEMENT SYMBOL Element Symbol Latin Name The symbol is the short form or Antimony Sb Stibium abbreviated name of the element. Each element has a chemical symbol that is Copper Cu Cuprum unique to it. For example, the symbol for Gold Au Aurum Iron Fe Ferrum carbon is C. Lead Pb Plumbum Many elements have their symbols Mercury Hg Hydragyrum derived from either the first letter or the Potassium K Kalium first two letters of their names. A few elements have symbols derived Silver Ag Argentum from their Latin names, as given in the Sodium Na Natrium Tin Sn Stannum table. (https://www.syvum.com/cgi/online/serve.cgi/squizzes/chem/periodic1b.html) Tungsten W Wolfram PREPARED BY: MS. ANN KIMBERLY S. MENDOZA PERIOD AND GROUP PREPARED BY: MS. ANN KIMBERLY S. MENDOZA PERIODS - 7 horizontal rows in the periodic table PERIOD 1 has 2 elements corresponding to 2 electrons in the s sublevel. Period 2 and 3 have 8 elements corresponding to 8 electrons in the s and p sublevels. Period 4 and 5 have 18 elements corresponding to 18 electrons in the s, p, and d sublevels. Period 6 has 32 elements corresponding to 32 electrons in the s, p, d and f sublevels. Period 7 is still incomplete but elements fill up s,p,d and f sublevels. PREPARED BY: MS. ANN KIMBERLY S. MENDOZA GROUPS/FAMILIES - vertical columns that are divided into A and B subgroups A GROUPS GROUP 1A- Alkali metals GROUP5A – Nitrogen Family GROUP 2A- Alkaline earth metals GROUP6A – Oxygen Family GROUP 3A- Boron Family GROUP 7A - Halogens GROUP 4A- Carbon family GROUP8A – Noble/ inert gases B GROUPS ARE THE TRANSITION ELEMENTS PREPARED BY: MS. ANN KIMBERLY S. MENDOZA PREPARED BY: MS. ANN KIMBERLY S. MENDOZA  CLASSIFICATION OF ELEMENTS Representative elements: column labeled 1A to 7A. The term representative elements refers to the stepwise addition of electrons to the s and p sublevels of the atom. NOBLE OR INERT GASES: the last group of the table (Group 8A). Each element has a completely filled set of s and p sublevels. They are colorless and exhibit little or no reactivity. Inert gases since they were once considered chemically unreactive. TRANSITION ELEMENTS: Columns 1B to 8B The group starts with 3B up to 8B, which has 8 columns, and then ends with 1B and 2B. These sequences, which contain 10 elements each, are related to the stepwise addition of the 10 electrons to the d sublevel of the atoms. INNER TRANSITION ELEMENTS: The two additional horizontal rows below comprise two groups of elements that were discovered to have similar characteristics: lanthanum in the 6th period, called lanthanide (rare earth elements are all metals), and actinium in the 7th period, called actinide (heavy rare elements are all radioactive). PREPARED BY: MS. ANN KIMBERLY S. MENDOZA PREPARED BY: MS. ANN KIMBERLY S. MENDOZA  POSITION OF ELEMENTS 1. For A family, the number of valence electrons (electrons in the outer energy levels) of the atoms of the elements in their respective groups correspond to their GROUP NUMBER. 2. The HIGHEST M A I N ENERGY LEVEL or the number of occupied main energy levels (m.e.l) by the electrons correspond to the PERIOD to which the element belongs. PREPARED BY: MS. ANN KIMBERLY S. MENDOZA 3. The element that belong to the same group have similar outer electronic configurations or last sublevel configurations (LSC). Thus, the periodic table can be divided into 4 blocks. 1. s-block (Groups 1A and 2A) – the LSC of these two groups are Ns1 and Ns 2 respectively where n represents the period number where the element belongs. 2. p-block (Groups 3A and 8A) – the characterized by stepwise addition of electrons to p sublevel. Thus the LSCs are Np 1 and Np 6 (except He which is 1s2 ) 3. d-block (Groups 3B and 2B) – the characterized by stepwise addition of electrons to d sublevel. Thus the LSCs are (n-1)d1 and (n-1)d10 4. f-block (Lanthanide and Actinide) – characterized by inner building of the f orbitals. Thus the LSCs are (n-2)f1 and (n-2)f14 PREPARED BY: MS. ANN KIMBERLY S. MENDOZA PREPARED BY: MS. ANN KIMBERLY S. MENDOZA  TYPE OF ELEMENTS Metals are located on the left side and in the center of the periodic table. About 80 elements are classified as metals, including some from every group except 7A and 8A. Atoms of metals tend to donate electrons; elements with three or fewer electrons in the outer energy level Metals have high densities, high melting temperatures, luster, and are good conductors of heat and electricity. Non-metals appear at the far right and toward the top. Atoms of non-metals tend to accept electrons in reaction with metals; elements have five or more electrons at the outer energy level. Non-metals have low densities, low melting temperatures are poor conductors of heat and electricity. Metalloids are borderline elements that, to some extent, exhibit both metallic and non-metallic properties. They usually act as donors with metals and electron acceptors with non-metals. These elements lie close to the zigzag line in the periodic table. PREPARED BY: MS. ANN KIMBERLY S. MENDOZA PREPARED BY: MS. ANN KIMBERLY S. MENDOZA  TRENDS IN PROPERTIES PREPARED BY: MS. ANN KIMBERLY S. MENDOZA  METALLIC PROPERTY refers to the ability of the atom to donate or give up electrons. ATOMIC SIZE IONIC SIZE When an atom loses or gains an electron, it becomes a positively or negatively charged particle ion. Metals lose electrons to form cations (positively charged ions), and non-metals gain electrons to form into anions (negatively charged). PREPARED BY: MS. ANN KIMBERLY S. MENDOZA  A non-metallic property is the ability of the atom to gain or accept electrons. Ionization energy is the amount of energy required to remove an electron from an atom or ion. A greater ionization energy is necessary to remove an electron from a positive ion as you go higher. Electron affinity refers to the energy released in the process of gaining electrons to form negative ions. Electronegativity is the ability of an atom in an element to attract or gain electrons. Metals are more electron donors, and non-metals are more electron acceptors. PREPARED BY: MS. ANN KIMBERLY S. MENDOZA PREPARED BY: MS. ANN KIMBERLY S. MENDOZA