History of the Periodic Table Essay

Explain how scientific observations led to the development of, and changes to, the hourly table. -Dmitri M destinationeleev- graduation exercise day-by-day table, organized 63 known elements according to properties, organized into rows and columns and wrote name, mass, and chemical substance properties on each -Julius Lothar Meyer- independently worked in Germany, sympathetic to Mendeleev -Henry Gwyn Jeffreys Moseley- Worked with Ernest Rutherford, experimented with 38 metals, he found that the positive charge of each elements nitty-gritty increased by one from element to element as they were pose in Mendeleevs periodic table, lead to modern definition of nuclear tally ( of protons in atoms nucleus) and the recognition the nuclear number was basis for organization of periodic table. name the organization of the modern periodic table.Arranged from left to right in rows (periods) by increasing atomic number and top to bottom in columns (groups) based on similar chemical propert iesLesson 03.02 assemblage Names and PropertiesComp be and contrast the properties of metals, metalloids, and nonmetals. -Metals- good conductors of ignite and electricity and reflect light and heat, more or less luster (shine) and most ar malleable (hammered or rolled into sheets) -Non-metals- poor conductors of heat and electricity, most are gas at room temperature, those that are solid are non malleable -Metalloids- a semiconductor (conduct electricity better than non-metals but non as good as metals), some characteristics of metals but more give care nonmetalsIdentify groups and sections of the periodic table by group name and familiar properties. 3.02 notesLesson 03.03 Periodic TrendsDescribe and develop the fashions for effective nuclear charge, atomic radius, dome radius, and ionization energy across a period and down a group. -Effective Nuclear Charge- the charge (from the nucleus) felt by the valence electrons after you convey taken into account the number of sh ielding electrons that surround the nucleus. -Atomic radius- half the remoteness  amidst the centers of two atoms of that element that are stayed together -Ionization Energy- the energy essential to remove one electron from an element, resulting in a positive ion. -Ionic radius- half the diameter of an ion.A positive ion is called a cation, and a negative ion is called an anion. Nonmetals usually become anions and metals usually become cations.Predict the properties of an element based on the known patterns of the periodic table. pulmonary tuberculosis periodic tableDescribe and explain the periodic trends for electron phylogenetic relation (honors). Electron affinity-The energy involved when a neutral atom gains an electron Becomes more negative (more energy is assumption off) for each element across a period from Group 1 to Group 17 because of an increase in effective nuclear charge. Becomes slight negative (more positive) going down a group, because each electron is being added to a higher energy level farther from the nucleus.Explain the exceptions to the trend across a period for ionization energy (honors). Noble gases in Group 18 all have positive electron affinity values. The noble gases must be forced to gain an electron because they already have a full valence energy level. The alkaline land metals in Group 2 and the nonmetals in Group 15 both have electron affinity values close to zero overdue to electron repulsion and effective nuclear charge. Nitrogen, in Group 15, does not form a stable -1 ion because when an additional electron is added to nitrogens valence energy level, it is added to a 2p orbital that already has one electron. The shoddy attracter amongst the added electron and nitrogens nucleus is wherefore there is not much energy tending(p) off.Lesson 03.04 Valence Electrons and stick toDefine and compare ionic and covalent bonding.-Ionic Bond- A chemical bond that results from electrostatic attraction between positive and negative ions, electrons are given up by one atom and gained by another atom, and past those atoms are attracted to each other.  among a metal and nonmetal. -Covalent bond- Electrons are shared between two atoms, neither atom completely gains or loses electrons. Between two nonmetals.Relate your knowledge of the periodic trends to the chemical bonding exhibited by various elements.Lesson 03.05 Ionic Bonding and Writing Formulas meet an elements ionic charge based on its location on the periodic table. Group 1- 1+Group 2- 2+Group 3- 3+Group 4- 4+Group 5- 3-Group 6- 2-Group 7- 1-Group 8- non-reactive noble gases drop a line the correct ionic regulation when given two elements that bond ionically. Use question above and periodic tableLesson 03.06 Covalent Bonding and Lewis Structures train how many covalent bonds an atom needs in order to subscribe its valence shell, using the periodic table. Must get to 8 pelmet electrons.Ex. Group 17 needs one more valance electron group 6 needs 2 more valance electrons haulage correct Lewis structures to model covalently bonded molecules when given the name or formula of the molecule.Describe your observations and conclusions from the virtual lab.Lesson 03.07 Intermolecular ForcesUse VSEPR theory to predict the shape of a molecule based on its Lewis structure. The VSEPR theory is about geometry of compounds and electron location. canvass and contrast intermolecular forces (capital of the United Kingdom dispersion, dipole-dipole, hydrogen bonding, and ion-dipole).London dispersion forces occur between all molecules and particles but are the altogether force of attraction between nonglacial molecules or noble gas atoms. These forces are the weakest of the intermolecular forces. The London dispersion forces are caused by the motion of electrons. Dipole-dipole forces are electrostatic interactions of permanent wave dipoles in polar molecules.The attractive forces that occur between the positive end of one polar molec ule and the negative end of another polar molecule tend to align the molecules to increase the attraction. Hydrogen bonding is a particularly strong dipole-dipole interaction in which hydrogen is covalently bonded to a passing electronegative element, and attracted to the very electronegative element in another molecule. It occurs only in molecules containing N-H, O-H or F-H bonds. Ion-dipole forces are attractive forces that result from the electrostatic attraction between an ionic compound and a polar molecule. This interaction is most commonly found in solutions, especially in solutions of ionic compounds in polar solvents, such as water.Identify the intermolecular forces experienced by different compounds. Intramolecular Forces The forces of attraction that occur between individual molecules.Lesson 03.08 denomination CompoundsCorrectly name covalent compounds, ionic compounds, and acids when given their formulas. A metal forms a positive ion (cation) and a nonmetal forms a neg ative ion (anion). The cation and anion assent to form an ionic compound, more specifically referred to as a double star ionic compound.Write the formulas for ionic compounds, covalent compounds, and acids from their names.Name furnishs or put out the formula of a hydrate when given its name (honors). Same prefixesLesson 03.09 mill Mass of CompoundsCalculate the molar mass of compounds from the formula. square up empirical formulas from per centum by mass or mass data.Empirical formula The formula of a compound in which the subscripts represent the lowest whole-number ratio of the atoms.Determine the molecular formula from the empirical formula and molar mass of a substance. No clueCalculate the molar mass of a hydrate and determine the formula of a hydrate from observational data (honors). H2O- 18.015Determine the empirical formula of a compound from the mass of the products produced in experimental reactions (honors).