Inorganic Chemistry Reviewer PDF - IPS 1 Module 1

Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh...

Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr PART 1. FUNDAMENTALS OF INORGANIC MASS Measure of the quantity of matter CHEMISTRY CHEMISTRY The science that describes matter—its properties, the changes it undergoes, and the energy changes that accompany those processes Matter - mass and volume The CENTRAL SCIENCE BRANCHES OF CHEMISTRY VOLUME ORGANIC CHEMISTRY Amount of space Hydrocarbons and its derivatives ENERGY The capacity to do work or to transfer heat ★ From the word itself, it has hydrogen > - kinesis-motion and carbons 1. Kinetic Energy ★ Ex: methane, ethane ➔ Energy in motion INORGANIC CHEMISTRY 2. Potential Energy ➔ Energy at rest Inorganic compounds, metals, minerals Energy Changes: ANALYTICAL CHEMISTRY ➔ Exothermic - release - (heat) ↳ palabas Detection and identification of substances ➔ Endothermic - absorbs present (qualitative analysis) or amount of each - (heat) - > 100b substance (quantitative analysis) BIOCHEMISTRY STATES OF MATTER Processes in living organisms PHYSICAL CHEMISTRY Behavior of matter ! BOARD EXAM QUESTION ! What is the property of Carbon that makes it possible to link by itself? ↳ expands indefinitely ↳ highly compressible CATENATION → Carbons can bind to another carbon, it’s almost infinite A1. MATTER MATTER AND ENERGY MATTER Anything that has mass and occupies space Kaedyne Rei 1  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr B. Sulfur is a yellow powder. C. A dry piece of paper burns. D. Pure water, for example, has a density of 0.998 g/cm3 at 25°C. EXTENSIVE & INTENSIVE PROPERTIES EXTENSIVE PROPERTIES Dependent on the amount of substance Formation of dry ice is an example of? - E.g. Mass - more substance, greater mass A. Sublimation ↳ solid carbon dioxide E.g. Volume - more substance, greater B. Freezing ( for + X. disease) eczema skin volume size , - C. Evaporation CO2 gas solid > - weight - D. Deposition g INTENSIVE PROPERTIES length - E. Condensation ↳ Independent on the amount of substance color luster - - What type of phase inversion does Naphthalene temperature - - hardness balls undergo? ↳ moth - E.g. Density boiling point/melting - A. Sublimation solid gas > - balls E.g. Electrical conductivity point B. Freezing ( for urinal , Naphthalene-lumilit pero C. Evaporation cabinet) D. Deposition walang liquid Which of the following is an EXTENSIVE property of E. Condensation formation matter? A. Hardness PHYSICAL & CHEMICAL PROPERTIES B. Size PHYSICAL PROPERTIES C. Melting point D. Color Can be observed or measured without changing the identity of the substance. e.g. color, hardness, melting point, boiling point Way to Tell Intensive & Extensive Properties Ex: H20 subjected to heat → H20 parin Take two identical samples of a substance and put Ex : ice cube na natural them together. CHEMICAL PROPERTIES If this doubles the property (e.g., twice the mass, Exhibited by matter as it undergoes twice as long), it's an extensive property. If the property is unchanged by altering the sample changes in composition. size, it's an intensive property. e.g. hydrogen has the potential to ignite and explode given the right PHYSICAL & CHEMICAL CHANGES conditions PHYSICAL CHANGE e.g. iron reacts with oxygen gas to No change in chemical composition form rust -) susunugin and paper ex: ignite (paper → ash) REVERSIBLE Ex; shredding paper, boiling of water, breaking a bottle CHEMICAL CHANGE Which of the following is a chemical property of matter? One or more substances are used up A. Silver is a shiny metal that conducts One or more new substances are electricity very well. formed Kaedyne Rei 2 PHASE CHANGES Gas to Liquid > - CONDENSATION Liquid to Gas > - EVAPORATION Gas to Solid - > DISPOSITION Solid to Gas-- SUBLIMATION Solid to Liquid-MELTING Liquid to Solid - FREEZING  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr Energy is absorbed or releases HETEROGENOUS MIXTURES > - multiple IRREVERSIBLE (Denaturation) Components are distinguishable Ex: burning of paper, cooking an egg, Multiple phases souring of milk Do NOT have same composition throughout (i.e. different amount in various areas) Which of the following exhibits a chemical change? e.g. SUSPENSION EMULSION , A. Ice cream melting COMPOUNDS B. Making a sand castle Can be decomposed to simpler C. A macbook falling out of window D. Fireworks exploding substance by chemical changes e.g. water, H2O can be broken into hydrogen and oxygen gases via electrolysis. NOTE: consists of atoms of two or more different A physical change may suggest that a elements bound together chemical change has also taken place. ELEMENTS ➔ Ex: naghalo ng two compounds, at Cannot be decomposed to simpler nagkaroon ng new color = chemical substance by chemical changes change Consists of only one kind of atom For instance, a color change, a warming, or the formation of a solid (ppt) when two solutions are mixed could indicate a chemical D change. CLASSIFICATION OF MATTER anic inorgi a multiple + ↳ suspensions ↳ Solutions (1 phase) 4 CANNOT be ↳ CAN be ↳ Emulsions decomposed decomposed CLASSIFICATION OF MATTER MIXTURE - HOMO/HETERO * Variable Composition (e.g. 70%, 80% or 95% ethanol in water) May be separated into pure substances by physical methods (e.g. distillation used & than 202 in more than 20 degcel, filtration) more PURE SUBSTANCE Fixed composition (e.g. 100% ethanol) Cannot be separated into simpler substances by physical methods Kaedyne Rei 3  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr HOMOGENOUS MIXTURES > - single Components are NOT distinguishable Single phrase Have some composition throughout (i.e X same amount in any areas) E.g. SOLUTION ↳ nuccers THE ATOMIC NUMBER (Z) The number of protons in the nucleus of an How would you categorize each example of atom determines its identity; this number is matter? (element, compound, homogeneous known as the atomic number of that element mixture, or heterogeneous mixture) Example: AN # of protons = - #20 pulp extract + + 1. Freshly squeezed orange juice - Heterogenous → Hydrogen contains 1 - proton 2. Red wine - Homogenous → Lithium atom contains 3 protons 3. Table salt - Compound THE MASS NUMBER (A) - Potal 4. Mercury - Element The mass number of an 5. Oxygen gas, O2 - Element atom is the sum of the number of protons and the number of neutrons in its nucleus; that is unders 𝑴𝒂𝒔𝒔 𝑵𝒖𝒎𝒃𝒆𝒓 = # 𝒐𝒇 𝒑 + # 𝒐𝒇 𝒏 A2. ATOM AND ITS ELECTRONIC STRUCTURE 𝑴𝒂𝒔𝒔 𝑵𝒖𝒎𝒃𝒆𝒓 = 𝑨𝒕𝒐𝒎𝒊𝒄 𝑵𝒖𝒎𝒃𝒆𝒓 + 𝑵𝒆𝒖𝒕𝒓𝒐𝒏 𝑵𝒖𝒎𝒃𝒆𝒓 > same THE ATOM - O ISOTOPES ATOM Isotopes are atoms of the same element with The smallest unit that retains the properties of different masses. an element They are atoms containing the same number of protons but different numbers of neutrons DALTON’S THEORY All matter is composed of atoms and these cannot be made or destroyed neutrons + protons -> O valence +1 - I Kaedyne Rei 4  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr NUCLIDE SYMBOL Note: Another way of representation for isotopes Represents the composition of the nucleus [Element name] - [Mass number] - mAss/p + n Determine the number of protons, neutrons and electrons in each of the following species. Are the members within each pair isotopes? ↳ atomic/protons ↳ same protons Note: Chemists often omit the subscripted atomic number because the element symbol implies the atomic number. To calculate the number of neutrons; No. 𝒐𝒇 𝑵𝒆𝒖𝒕𝒓𝒐𝒏𝒔 = 𝑴𝒂𝒔𝒔 𝑵𝒖𝒎𝒃𝒆𝒓 − 𝑨𝒕𝒐𝒎𝒊𝒄 𝑵𝒖𝒎𝒃𝒆𝒓 QUESTION Calculate the number of neutrons in the given isotopes of carbon Kaedyne Rei 5  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 (smalleratom rr Solid Sphere (Billiard ball) Model subatomic Atom as solid sphere but NOT indivisible (subatomic particle, called “quarks”) 1964 > - Dalton dismissed Leucippus and Democritus’ claims - samemuss a i DISCOVERY OF ELECTRONS HUMPHRY DAVY (1800s) Elements of a chemical compound are held = G = G together by electrical forces MICHAEL FARADAY Relationship between the amount of electricity used in electrolysis and the amount of chemical THE ATOMIC WEIGHT reaction that occurs↳ He0 Many elements occur in nature as mixtures of GEORGE STONEY (1891) isotopes. “Electrons” → Electic ions The atomic weight of such an element is the ↳ Electric weighted average of the masses of its isotopes. DISCOVERY OF ELECTRONS Atomic weights are fractional numbers, not CATHODE-RAY TUBE EXPERIMENT integers Joseph John Thomson (1897) /JJ Thomson e The “most convincing evidence” of electrons = p Thomson discovered “Electrons” 21-10 - MODELS: - J.. J 1. Plum Pudding Model - - → (-) charged particles embedded in the sea of (+) charge 2. Oil-drop Experiment → Robert Millikan (1909); Determine the - oil A3. DEVELOPMENT OF ATOMIC MODELS charge of electrons Kelangan ng mo para gumawa ng milk 3. Saturn-like model EARLY HISTORY O Nagaoka (1903) → Hantaro ↳ turn-Saturn LEUCIPPUS AND DEMOCRITUS DISCOVERY OF PROTONS Greek word “Atomos” - uncuttable Atom as a solid indivisible sphere CANAL RAYS EXPERIMENT ARISTOTLE AND OTHERS > - may gold sa Canal Matter is made up of four elements Eugen Goldstein (1886) - Earth, water, air, and fire Cathode-ray tube also generates a stream of positively charged particles DALTON’S ATOMIC THEORY JOHN DALTON (1807) Kaedyne Rei 6  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr These positive rays, or positive ions, are THE DISCOVERY OF NEUTRONS created when the gaseous atoms in the tube JAMES CHADWICK (1932) lose electrons. Bombardment of beryllium with Squatter (Scattering MODELS: - Si Ruth ay and ugali high-energy alpha- particles produced 1. Rutherford’s Model - NEUTRONS → The Scattering Experiment DISCOVERED NEUTRONS Ernest Rutherford (1910) He discovered “protons” MODELS: BOR - 1. g > planetary model BOHR’S MODEL - Aut Niel’s Bohr - described the electron of a hydrogen atom as revolving around its nucleus in one of a discrete set of circular orbits Bohr’s Planetary Model ➔ Each orbit thus · corresponds to a definite energy level for the electron. ➔ When an electron is ASSUMPTION excited from a lower If the Thomson model of the atom were energy level to a higher correct, any alpha-particles passing one, it absorbs a definite through the foil would have been (quantized) amount of deflected by very small angles. energy. Quite unexpectedly, nearly all of the a-particles ➔ Electrons occupy only passed through the foil with little or no certain energy levels in deflection atoms RUTHERFORD’S CONCLUSION Atoms consist of very small, very dense positively charged nuclei surrounded by clouds of electrons at relatively large distances from the nuclei 2. Nuclear Model THE WAVE NATURE OF ELECTRONS Positive charge localized in the nucleus LOUIS DE BROGLI Proposed the idea of wave-like nature of ATOMIC NUMBER OF AN ELEMENT electrons Electrons can be treated as waves more HENRY GWYN JEFFREYS MOSELEY(1913) /HGJ effectively than as small compact particles He studied X-Rays given off by various traveling in circular or elliptical orbits. elements “The number of protons in the nucleus of an QUANTUM MECHANICS atom determines its identity; this number is known as the atomic number of that element.” QUANTUM MECHANICS At Mass Based on the wave properties of matter Z 2) Atomic Kaedyne Rei 7  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr WERNER HEISENBERG’S UNCERTAINTY ANGULAR MOMENTUM QUANTUM NUMBER PRINCIPLE (1927) > agreed to Louis - a.k.a. Azimuthal or Orbital Angular For electrons, it is not possible to determine the momentum Quantum Number exact momentum and the exact position at the 𝒍 = 𝟎, 𝟏, 𝟐, 𝟑, … (𝒏 − 𝟏) same moment in time Orbital SUBSHELL/ SUBLEVEL Shape of the orbital ★ The mathematical approach of quantum mechanics involves treating the electron in - 𝒍=𝟎 s spherical an atom as a standing wave - 𝒍=𝟏 p dumb-bell ERWIN SCHRODINGER’S WAVE EQUATION - 𝒍=𝟐 d clover leaf It estimates the position of electrons and - 𝒍=𝟑 f complex quantifies energy levels ATOMIC ORBITALS (Erwin Schrodinger) A region of space in which the probability of finding an electron is high MODERN ATOMIC MODEL Erwin Schrodinger ★ Electron Cloud Model O ★ Quantum Mechanical Model i A4. QUANTUM NUMBERS O QUANTUM NUMBERS Each atomic orbital is described by a set of O quantum numbers. O 1. Principal QN (𝒏) (n) (1) ( mi) ( ms) 2. Orbital QN (𝒍) POMS O 3. Magnetic QN (𝒎𝒍) n 4. Spin QN (𝒎𝒔) - for individual electrons only MAGNETIC QUANTUM NUMBER PRINCIPAL QUANTUM NUMBER 𝒎𝒍 = −𝒍 … 𝟎 … + 𝒍 > integers - 𝒏 = 𝟏, 𝟐, 𝟑, … (𝒏) Orbital → Specific orbital Orbital SHELL or ENERGY LEVEL Orientation in space of the orbital Distance of the electron from the nucleus Higher 𝒏, higher energy - - - - L - - - - - - - SPIN QUANTUM NUMBER Kaedyne Rei 8  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr Fi PREDICTING ELECTRON CONFIGURATION OF AN ATOM AUFBAU PRINCIPLE * Orbitals fill in order of increasing energy, from Ex : (n , 1 , and m1) in a 3p subshell lowest to highest n= 3 (n = 1 2 , , 3 )... 1 = 1 (p = 1) > - psubshell S = 2 ml = - 1 , 0, + 1 (because 1 is 1) p = 6 d = 10 f = 14 ↓ energy 1522522p43523p - - 45236104p 592 * 4d" PAULI 5p"6s24f14 [ EXCLUSION PRINCIPLE No more than two electrons can occupy each orbital, and if two electrons are present, they A5. ELECTRON CONFIGURATION must have opposite spins. I In one subshell , no more than two can occupy ELECTRON CONFIGURATION > SPECIFIC - Electron in the outermost shell “Distribution of electrons” ↓ (VALENCE ELECTRON Describes the number and arrangement of Write the FULL electron configuration for electrons in orbitals, subshells and shells in sodium atom 2 2 6 + + = 10 lang kulang 3sO 1 Since 1s 2s 2p g na 2 21 6 > - ↳ e 11 an atom. = ↳ Valence Ground state election - Atom in its lowest energy, or unexcited, Write the FULL electron configuration for calcium atom state 1s22s22p63s23p600 4s2 ↳ Valence Electron ORBITAL DIAGRAMS Another way to represent the order of fill for an atom is by using an orbital diagram often referred to as "the little boxes" Kaedyne Rei 9  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 Ex in Exam : rr n 2 , 0 , 0 , + /2 Yes n , 1 , m) , ms # ! t 8 O - - 10 +1 - - = 0 n= 2 S= > - 2 10 +1 2 : - - + l = 1 O m1 : 0 - 3 - 2 - 10 +1 + 2 + y ms = + /(t) WRITING AN ORBITAL DIAGRAMS 34 54 12 HUND’S RULE The order of fill is the same but as you can see from above the electrons are placed singly into the boxes before filling them with both electrons. > - EX A single electron will occupy an empty orbital first before pairing > - SIMPLIFIED NOTATION: NOBLE GAS i 14 ++↓ / ** * - Est fill d) theempy CONFIGURATION - 2 - 10 + 1 + 2 An atom consists of the elemental symbol of the last noble gas prior to that atom, followed by the configuration of the remaining electrons. 3 MEMORIZE 0= S - 1 pr = 2 I = 3 = - mi = - 1... 0.. + l (nag stop sa-1) O - MS Kaedyne Rei 10  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr A6. THE PERIODIC TABLE OF ELEMENTS DMITRI MENDELEEV Based on chemical properties LOTHAR MEYER Based on physical properties → Both emphasized the periodicity, or regular periodic repetition of properties with increasing atomic weight. → Elements are now arranged in the periodic table in order of increasing atomic number PERIODIC LAW “The properties of the elements are periodic functions of their atomic numbers.” Vertical Columns → Groups or Families Horizontal Rows → Periods * volatile Met als ~ - = 18 - WRITING THE ELECTRON CONFIGURATION USING THE PERIODIC TABLE Nitrogenp O goxygen * ~ *2b - volatile metals ↓ Azote (no life) - G * Note : If it reaches & subshell (K) then minus the Blue-s-subshell Ex : Potassium energy level - yellow-p-subshell 1522522p3923p4s' Ex : Sc[3d'] Red-e-subshell [Ar] 4sI White-f-subshell Kaedyne Rei 11  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr ELECTRONEGATIVITY (EN) Measure of the relative tendency of an atom to attract electrons to itself when it is chemically combined with another atom => doesnot allowheat/electition QUESTION METALLOIDS Show some properties that are Which of the following element is the most characteristic of both metals and electronegative? non-metals A. Ca Semiconductors B. B ★ insulators at lower temperatures C. I but become conductors at higher D. F temperatures ★ silicon, germanium, and antimony PERIODIC PROPERTIES OF ELEMENTS ATOMIC RADII (SIZE) Defined as half of the distance between the nuclei of neighboring atoms in the pure element Expressed in Angstroms (1Å = 10-10 m) IONIZATION ENERGY (IE) The energy required to remove an electron from a gas-phase atom ↳ Noble gas (stable) ELECTRON AFFINITY (EA) The energy change that occurs when an electron is attached to an atom in the gas phase to form an negative ion Kaedyne Rei 12  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr PART 3. INORGANIC QUALITATIVE ANALYSIS SEPARATION OF CATIONS INTO ANALYTICAL GROUPS Certain ions easily dissolve, others tend to be insoluble. They all follow certain rules. We can use these rules in order to predict what ions are present in an ‘unknown’ solution (SUMMARY Group 1-5 Ex : > - 10 pts +2 Fe #I Py +2 It NHyt - -I , - v +2 I - 20 Mg + 2 v CD + 2 - I - + 2 So - # Sn +2 -IV +2 Ca E Ag + I - - Kaedyne Rei 20  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr pag nilagay malamig ja - Red > - Col ions -ppt - ATOM FLAME TEST An analytical method used for detecting the presence of certain metals where a small amount of a substance is volatilized and the characteristic glow of the substance is observed. CONFIRMATORY TESTS Non-luminous - Blue * Luminous-yellow O - F -where's solutions are volatilized Kaedyne Rei 21  Inorganic chemistry ❁ SEMESTER 1 IPS 1 - | MODULE 1 | PROF. Kyle Christian Vreeland, RPh SY. 2024-2025 rr FLAME TESTS Crimson - & I the cobalt glass absorbs & radiation from Na (N N) - (Krimson (cal) (per St ). (B B) - Note : * Lisr-carmine red , Crimson red A Sogo-sodium - Golden Yellow det * A(potassium) ↓ BaBCu-Ba(Yellow B (Green) Cu (Blue) Kaedyne Rei 22