Explain how scientific observations led to the development of. and alterations to. the periodic tabular array. -Dmitri Mendeleev- first periodic tabular array. organized 63 known elements harmonizing to belongingss. organized into rows and columns and wrote name. mass. and chemical belongingss on each -Julius Lothar Meyer- independently worked in Germany. similar to Mendeleev -Henry Gwyn Jeffreys Moseley- Worked with Ernest Rutherford. experimented with 38 metals. he found that the positive charge of each element’s karyon increased by one from component to element as they were arranged in Mendeleev’s periodic tabular array. lead to modern definition of atomic figure ( # of protons in atom’s karyon ) and the acknowledgment the atomic figure was footing for organisation of periodic tabular array.
Describe the organisation of the modern periodic tabular array.
Arranged from left to compensate in rows ( periods ) by increasing atomic figure and top to bottom in columns ( groups ) based on similar chemical belongingss
Lesson 03. 02: Group Names and Properties
Compare and contrast the belongingss of metals. metalloids. and nonmetals. -Metals- good music directors of heat and electricity and reflect visible radiation and heat. most luster ( radiance ) and most are ductile ( hammered or rolled into sheets ) -Non-metals- hapless music directors of heat and electricity. most are gas at room temperature. those that are solid are non ductile -Metalloids- a semiconducting material ( conduct electricity better than non-metals but non every bit good as metals ) . some features of metals but more like nonmetals
Identify groups and subdivisions of the periodic tabular array by group name and common belongingss. 3. 02 notes
Lesson 03. 03: Periodic Tendencies
Describe and explicate the tendencies for effectual atomic charge. atomic radius. ionic radius. and ionisation energy across a period and down a group. -Effective Nuclear Charge- the charge ( from the karyon ) felt by the valency negatrons after you have taken into history the figure of screening negatrons that surround the karyon. -Atomic radius- half the distance between the centres of two atoms of that component that are bonded together -Ionization Energy- the energy required to take one negatron from an component. ensuing in a positive ion. -Ionic radius- One-half the diameter of an ion.
A positive ion is called a cation. and a negative ion is called an anion. Nonmetals normally become anions and metals normally become cations.
Predict the belongingss of an component based on the known forms of the periodic tabular array. Use periodic tabular array
Describe and explicate the periodic tendencies for negatron affinity ( awards ) . Electron affinity-The energy involved when a impersonal atom additions an negatron Becomes more negative ( more energy is given off ) for each component across a period from Group 1 to Group 17 because of an addition in effectual atomic charge. Becomes less negative ( more positive ) traveling down a group. because each negatron is being added to a higher energy degree further from the karyon.
Explain the exclusions to the tendency across a period for ionisation energy ( awards ) . Baronial gases in Group 18 all have positive negatron affinity values. The baronial gases must be forced to derive an negatron because they already have a full valency energy degree. The alkalic Earth metals in Group 2 and the nonmetals in Group 15 both have electron affinity values near to zero due to electron repulsive force and effectual atomic charge. Nitrogen. in Group 15. does non organize a stable -1 ion because when an extra negatron is added to nitrogen’s valency energy degree. it is added to a 2p orbital that already has one negatron. The weak attractive force between the added negatron and nitrogen’s karyon is why there is non much energy given off.
Lesson 03. 04: Valence Electrons and Bonding
Define and compare ionic and covalent bonding.
-Ionic Bond- A chemical bond that consequences from electrostatic attractive force between positive and negative ions. negatrons are given up by one atom and gained by another atom. and so those atoms are attracted to each other. Between a metal and nonmetal. -Covalent bond- Electrons are shared between two atoms. neither atom wholly additions or loses negatrons. Between two nonmetals.
Associate your cognition of the periodic tendencies to the chemical bonding exhibited by assorted elements.
Lesson 03. 05: Ionic Bonding and Writing Formulas
Determine an element’s ionic charge based on its location on the periodic tabular array. 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 baronial gases
Write the right ionic expression when given two elements that bond ionically. Use inquiry above and periodic tabular array
Lesson 03. 06: Covalent Bonding and Lewis Structures
Determine how many covalent bonds an atom demands in order to make full its valency shell. utilizing the periodic tabular array. Must acquire to 8 cornice negatrons.
Ex. Group 17 needs one more cornice negatron ; group 6 needs 2 more cornice negatrons
Draw correct Lewis constructions to pattern covalently bonded molecules when given the name or expression of the molecule.
Describe your observations and decisions from the practical lab.
Lesson 03. 07: Intermolecular Forces
Use VSEPR theory to foretell the form of a molecule based on its Lewis construction. The VSEPR theory is about geometry of compounds and electron location.
Compare and contrast intermolecular forces ( London scattering. dipole-dipole. H bonding. and ion-dipole ) .
London scattering forces occur between all molecules and atoms but are the lone force of attractive force between nonionic molecules or baronial gas atoms. These forces are the weakest of the intermolecular forces. The London scattering forces are caused by the gesture of negatrons. Dipole-dipole forces are electrostatic interactions of lasting dipoles in polar molecules.
The attractive forces that occur between the positive terminal of one polar molecule and the negative terminal of another polar molecule tend to aline the molecules to increase the attractive force. Hydrogen bonding is a peculiarly strong dipole-dipole interaction in which H is covalently bonded to a extremely negatively charged component. and attracted to the really negatively charged component in another molecule. It occurs merely in molecules incorporating N-H. O-H or F-H bonds. Ion-dipole forces are attractive forces that result from the electrostatic attractive force between an ionic compound and a polar molecule. This interaction is most normally found in solutions. particularly in solutions of ionic compounds in polar dissolvers. such as H2O.
Identify the intermolecular forces experienced by different compounds. Intramolecular Forces: The forces of attractive force that occur between single molecules.
Lesson 03. 08: Naming Compounds
Correctly name covalent compounds. ionic compounds. and acids when given their expressions. A metal forms a positive ion ( cation ) and a nonmetal signifiers a negative ion ( anion ) . The cation and anion combine to organize an ionic compound. more specifically referred to as a binary ionic compound.
Write the expression for ionic compounds. covalent compounds. and acids from their names.
Name hydrates or compose the expression of a hydrate when given its name ( awards ) . Same prefixes
Lesson 03. 09: Molar Mass of Compounds
Calculate the molar mass of compounds from the expression.
Determine empirical expressions from per centum by mass or mass informations.
Empirical expression: The expression of a compound in which the inferiors represent the lowest whole-number ratio of the atoms.
Determine the molecular expression from the empirical expression and molar mass of a substance. No hint
Calculate the molar mass of a hydrate and find the expression of a hydrate from experimental informations ( awards ) . H2O- 18. 015
Determine the empirical expression of a compound from the mass of the merchandises produced in experimental reactions ( awards ) .
