Inorganic Chemistry Flashcards

Scientific method and Inorganic chemistry

Ion charged atom Ionic bond attraction between oppositely charged ions + ion (cation) Forms when an electron is lost – ion (anion) Forms when an electron is gained non polar covalent bond forms by the even sharing of electrons between atoms polar covalent bond forms by the uneven sharing of electrons between atoms Hydrogen bond […]

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Organic and inorganic chemistry

ionic bond A chemical bond resulting from the attraction between oppositely charged ions. Metal+ Non metal covalent bond A chemical bond formed when two atoms share electrons . Non metal + Non metal polar covalent bond unequal sharing of electrons non polar covalent bond equal sharing of electrons hydrogen bond A type of weak chemical […]

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chapter 2 inorganic chemistry

organic molecules they contain carbon-carbon covalent bonds or carbon-hydrogen covalent bonds. Inorganic do not. inorganic molecules water and some acids, bases, and salts water solvent (liquid into which solutes are dissolved) dehydration synthesis chemical reaction in which water is removed from small molecules so they can be strung together to form a larger molecule hydrolysis […]

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Inorganic chemistry crossword puzzle

ionic bonds where an element acquires an electron and the other element losses an electron are termed ___ bonds seven pH of a neutral solution None number of neutrons in a typical hydrogen atom aldehyde This functional group has a double bond oxygen with a terminal carbon Eight Maximum number of electrons that the second […]

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Inorganic vs Organic Chemistry

Organic chemistry Study of molecules that contain carbon compounds Inorganic chemistry Study of all compounds that do not contain carbon compounds Key differences between organic and inorganic chemistry Chemical structure Chemical classification Scientific purpose Chemical structure The main difference between organic and inorganic chemistry Organic compounds: – must contain a carbon atom in its structure […]

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Inorganic Chemistry- COMMON Names of Chemicals

Grain alcohol Ethyl alcohol or ethanol C2H5OH Wood alcohol Methyl alcohol or methanol CH3OH Ammonia water Ammonium hydroxide solution NH4OH Aqua Fortis Eau forte Aqua Fuerte Concentrated nitric acid HNO3 Aqua Regia 1 part Nitric acid + 3 parts Hydrochloric acid Baking soda Sodium bicarbonate NaHCO3 Baryte Barium hydroxide Ba(OH)2 Bauxite Impure Aluminum oxide Al2O3 […]

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Inorganic Chemistry Test 1

• Haber-bosh Process o Process that uses Fe-based inorganic catalysts to promote NH3 (ammonia) production • Ziegler Natta polymerization o Process used in polymer production (such as polyethylene) • Rydberg formula o Delta(E) = Rh*(1/ni^2-1/nf^2). Constitutes the emission spectrum of hydrogen • Schrödinger equation o Describes wave properties of electron in terms of position, mass, […]

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Inorganic Chemistry Final Review

Chemistry The study of the composition, structure, and properties of matter, the processes that matter undergoes, any energy changes that accompany these processes Organic chemistry The study of most carbon containing compounds Inorganic chemistry The study of non-organic substances, many of which have organic fragments bonded to metals Physical chemistry The study of the properties […]

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Biology 103 Inorganic Chemistry

matter Anything that takes up space and has mass matter Consists of chemical elements in pure form and in combinations and is composed of incredibly tiny particles called atoms and molecules Element A substance that cannot be broken down to other substances by ordinary chemical reactions. Today we recognize____ elements that occur naturally in nature. […]

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Inorganic Chemistry – Exam 1

Chemical A substance that has the same composition and properties wherever it is found. Chemistry The study of the composition, structure, properties, and reactions of matter. Conclusion An explanation of an observation that has been validated by repeated experiments that support a hypothesis. Experiment A procedure that tests the validity of a hypothesis Hypothesis An […]

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Inorganic Chemistry Exam 3

tetrahedral void 0.225r octahedral void 0.414r cubic void 0.732r Polymorphism The ability to adopt different crystal forms under different conditions of pressure and temperature Alloy Blend of metallic elements prepared by mixing molten components and then cooling to produce a solid Interstitial solid solutions Formed between metals and small atoms that can occupy voids while […]

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Inorganic Chemistry (Chapter 2)

Covalent Bond Formed when two neighboring atoms share an electron pair. Single Bond A shared electron pair. Double Bond Two shared electron pairs. Lone Pair An unshared pair of valence electrons on an atom. Octet Rule Each atom shares electrons with neighboring atoms to achieve a total of eight valence electrons. Lewis Structure A diagram […]

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ENVS test 2 pt 2- Inorganic Chemistry

inorganic chemistry non-carbon containing compounds What is the most important compound on earth? water Polar slightly positive one side, slightly negative side. -attract ions Universal Solvent readily forms solutions with other polar molecules and ions allowing it to dissolve and suspend numerous substances Cohesive sticks to things Resistance to temperature change high amount of energy […]

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Biology Unit 1 – Inorganic Chemistry

Atomic number The number of protons in an atom mass number (atomic mass) number of protons plus the number of neutrons in an atom Ion An atom that carries either a positive or a negative charge. An ion is formed when the number of e’ is not equal to the number of protons in the […]

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Unit 2 Inorganic Chemistry-Biology

Inorganic does not contain carbon and hydrogen element substance that cannot be separated into a simpler substance; examples: carbon, oxygen, gold. atom the smallest portion of an element proton (+) positively charged subatomic particle located in the nucleus neutron neutrally (0) charged subatomic particle located in the nucleus electron negatively(-) charged subatomic particle located outside […]

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Acid-Base Inorganic Chemistry (Chapter 6)

Arrhenius Acid PRODUCES H+ (H₃O+ ions) Arrhenius Base PRODUCES OH- Bronsted-Lowry Acid H+ DONOR Bronsted-Lowry Base H+ ACCEPTOR Bronsted-Lowry general Acid-Base reaction focuses on what? Transfer of H+ (Focuses on H+ moving around) Deprotonation Loss of a proton Conjugate Acid Has an extra H+ (Example: NH₄⁺ is the conjugate acid of NH₃) Conjugate Base Lost […]

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Inorganic chemistry and the periodic table

Positive test for decomposition of nitrates Brown toxic gas/ glowing splint is relit Disproportionation An element in a single species being simultaneously oxidised and reduced Ionisation energy …… down Group 2 Decreases Ionic precipitation reaction Reaction producing a solid precipitate when 2 solutions are mixed that contain ions Charge or group 2 element ions 2+ […]

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Inorganic chemistry

Group 7: boiling points Increases down group- vdwfs increases due to increase in size and increase in Relative atomic mass. Group 7: electronegativity Decreases down group due to increase in shielding Group 7: displacements – oxidising strength decreases down ground cos of electron increase – electrons with smaller radius Periodicity: Atomic radius – increases across […]

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Inorganic Chemistry – Acids, Bases, and Buffers

pH a measure of the concentration of hydrogen ions in a solution Alkalinity a quantitative measurement of the ability of an aqueous solution to neutralize an acid. The 2 ions produced by the ionization of water are: Hydroxide (OH-) and Hydronium (H3O+) Ionization of water formula: 2(H2O)H3O+ + OH- Simplified Ionization of water formula: H2O […]

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Inorganic Chemistry: Coordination Chemistry

Crystal Field Theory Designed for coordination compounds: Ligands+ Metal ion (+charge) Orbital Energy Determined by ligand number, compound structure, and electric field strength of ligands Nucleophilicity order of ligands 1. Across a row: C⁻>N⁻>O⁻>F⁻ since increasing electronegativity decreases the lone pair availability. 2. Comparing same atom: higher electron density increases nucleophilicity (HO⁻>H₂O) 3. Within a […]

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Physical and inorganic chemistry chapter 2 stoichiometry

Avogadro’s number 6.022 x 10^23. example: 1 mol of C =6.022 x 10^23, 1 mol of HCl= 6.022 x 10^23, 2 mol of NaCl= 2 x 6.022 x 10^23 Number of Cl- ions in 2 moles of MgCl2 = 2 x 2 x 6.022 x 10^23 Number of Mg2+ ions in 1 mol of MgCl2 […]

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