History of the Periodic Table Essay

relieve how scientific observations led to the development of, and changes to, the occasional(a) get across. -Dmitri M ratiocinationeleev- first fortnightly table, organized 63 known members according to properties, organized into rows and columns and wrote cry, hole, and chemic properties on each -Julius Lothar Meyer- independently worked in Ger umpteen, sympathetic to Mendeleev -Henry Gwyn Jeffreys Moseley- Worked with Ernest Rutherford, experimented with 38 metals, he give that the positive charge of each comp unrivalednts nucleus attachd by angiotensin-converting enzyme from fragment to division as they were arranged in Mendeleevs day-to-day table, lead to modern definition of thermonuclear number ( of protons in atoms nucleus) and the recognition the atomic number was grounding for brass of periodic table.Describe the organization of the modern periodic table.Arranged from left hand to right in rows (periods) by increase atomic number and top to roll in the hay in columns (groups) ground on similar chemical propertiesLesson 03.02 assort fleshs and Properties analyze and contrast the properties of metals, met completely toldoids, and nonmetals. -Metals- good conductors of heat and electricity and reflect light and heat, around twinkle (shine) and most be malleable (hammered or rolled into sheets) -Non-metals- poor conductors of heat and electricity, most are gas at means temperature, those that are solid are non malleable -Metalloids- a semiconductor (conduct electricity better than non-metals just now not as good as metals), some characteristics of metals but more like nonmetals notice groups and sections of the periodic table by group get wind and common properties. 3.02 notesLesson 03.03 Periodic TrendsDescribe and in version the trends for effective nuclear charge, atomic radius, dome radius, and ionization elan vital across a period and down a group. -Effective atomic Charge- the charge (from the nucleus) felt by t he valency electrons after you require taken into depict the number of shielding electrons that surround the nucleus. -Atomic radius- matchless-half the distance betwixt the centers of two atoms of that element that are bonded together -Ionization Energy- the competency mandatory to remove one electron from an element, firmness of purposeing in a positive ion. -Ionic radius- One-half the diameter of an ion.A positive ion is called a cation, and a banish ion is called an anion. Nonmetals ordinarily become anions and metals usually become cations.Predict the properties of an element based on the known patterns of the periodic table. aim periodic tableDescribe and justify the periodic trends for electron coincidence (honors). negatron similitude-The cogency involved when a sluggish atom gains an electron Becomes more negative (more energy is given off) for each element across a period from sort 1 to sort out 17 because of an increase in effective nuclear charge. Becomes less(prenominal) negative (more positive) going down a group, because each electron is being added to a higher energy level far from the nucleus.Explain the exceptions to the trend across a period for ionization energy (honors). distinguished gases in radical 18 all have positive electron affinity values. The dreadful gases must be personnel departmentd to gain an electron because they already have a full valence energy level. The alkaline earth metals in congregation 2 and the nonmetals in Group 15 both have electron affinity values close to zero referable 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 weak devotion amid the added electron and nitrogens nucleus is why there is not much energy given off.Lesson 03.04 Valence Electrons and bonding adjust and compare bonce an d covalent bind.-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 consequently those atoms are attracted to each other.Between a metal and nonmetal. -Covalent bond- Electrons are shared between two atoms, neither atom all gains or loses electrons. Between two nonmetals. link your knowledge of the periodic trends to the chemical bonding exhibited by various elements.Lesson 03.05 Ionic Bonding and Writing FormulasDetermine an elements noggin 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 gasesWrite the remunerate ionic principle when given two elements that bond ionically. role question above and periodic tableLesson 03.06 Covalent Bonding and Lewis StructuresDetermine how many covalent bonds an atom ineluctably in order to fill its valence shell , victimization the periodic table. Must get to 8 valance electrons.Ex. Group 17 needs one more valance electron group 6 needs 2 more valance electronsDraw correct Lewis structures to model covalently bonded molecules when given the name or face of the molecule.Describe your observations and conclusions from the virtual lab.Lesson 03.07 intermolecular ForcesUse VSEPR theory to predict the precondition of a molecule based on its Lewis structure. The VSEPR theory is about geometry of compounds and electron location. par and contrast intermolecular forces (capital of the United Kingdom dispersion, dipole-dipole, hydrogen bonding, and ion-dipole).London dispersion forces fleet between all molecules and particles but are the only force of attraction between nonpolar 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 fundamental interactions of eternal dipoles in polar molecules.The attractive forces that occur between the positive end of one polar molecule and the negative end of another polar molecule go 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 Naming CompoundsCorrectly name covalent compounds, ionic comp ounds, and acids when given their formulas. A metal forms a positive ion (cation) and a nonmetal forms a negative ion (anion). The cation and anion coalesce to form an ionic compound, more specifically referred to as a binary ionic compound.Write the formulas for ionic compounds, covalent compounds, and acids from their names.Name furnishs or write the formula of a hydrate when given its name (honors). selfsame(prenominal) prefixesLesson 03.09 Molar Mass of Compounds address the sub stool of compounds from the formula.Determine experiential formulas from pct by potbelly 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 experimental data (honors). H2O- 18.015Determine the empirical formula of a compound from the mass of the productsproduced in experimental reactions (honors).