STM 005 General Chemistry 1 2nd Quarter PDF

EXPLORING LIMITING REACTANT AND PERCENT YIELD STM 005 (SAS 15) KAAGAPAY SWUDENTS CIRCLE LIMITING REAGENT a chemical reactant that limits the amount of product that is formed the limiting reagent gives the smallest yield of product calculated from the...

EXPLORING LIMITING REACTANT AND PERCENT YIELD STM 005 (SAS 15) KAAGAPAY SWUDENTS CIRCLE LIMITING REAGENT a chemical reactant that limits the amount of product that is formed the limiting reagent gives the smallest yield of product calculated from the reagents (reactants) available this smallest yield of product is called the theoretical yield The other reactant that is not completely consumed in the reaction is called the excess reactant. DESCRIBING THE PROPERTIES OF GASSES STM 005 (SAS 16) KAAGAPAY SWUDENTS CIRCLE PROPERTIES move randomly (elastic collisions, bounce when hit things like billiard balls, very fast, flow), can be compressed(not attracted to each other, spread out as far as possible to fill space, no definite shape or volume) KINETIC MOLECULAR THEORY A. a gas consist of very small particles THEORETICAL YIELD B. the particles are in constant, random, straight- line motion C. the molecules of a gas are very far from the maximum amount of product which each other could be produced by the complete reaction D. there are no forces of attraction or repulsion of the limiting reactant between molecules E. molecules collide with each other and with ACTUAL YIELD the walls of the container F. all collisions are perfectly elastic the amount of product formed from the actual chemical reaction and is usually less TEMPERATURE than the theoretical yield the measure of the average kinetic energy PERCENT YIELD of the particles in an object K = oC + 273.15 (The absolute temperature of a gas is a the percent of the product formed based measure of the average kinetic energy of its upon the theoretical yield molecules)  directly GAS PRESSURE proportional Temperature when mass and must be in pressure are kelvin. K = oC defined as force per unit area (P= F/A). SI kept constant. + 273 unit of pressure is newton’s per square meter (N/m2) Gay-Lussac’s Temperature & 𝑃1 𝑃2 this unit is also called pascal (Pa). Another Law pressure are 𝑇1 = 𝑇2 unit of pressure is millimeters mercury directly (mmHg) proportional if one millimeter mercury is also called torr mass & volume the standard temperature and pressure are kept (STP) is the condition where the constant. temperature is 273.15 K and the pressure is 1 atm Avogadro’s The volume of a 𝑉1 𝑉2 = Law gas at constant 𝑛1 𝑛2 ATMOSPHERIC PRESSURE temperature and pressure is directly caused by the collisions of air (gas) proportional to molecules the amount of gas expressed Standard pressure conversion: 1 atm = in moles, 101.3kPa = 760 mmHg VAPOR PRESSURE Combined describes the 𝑃1𝑉1 𝑃2𝑉2 = Gas Law relationship 𝑇1 𝑇2 gas collision in a sealed container, liquid among the going to gas, gas going to liquid, reaches pressure, equilibrium when temperature remains volume and constant, increase the temperature will temperature of a increase the pressure in a sealed container constant amount of gas. GAS LAWS Ideal Gas from which 𝑃𝑉 = 𝑛𝑅𝑇 Law simpler gas laws simple mathematical relationships between such as Boyle's, volume, pressure, temperature, and amount Charles's, of a gas Avogadro's and Gay Lussac’ s GAS LAW DEFINITION FORMULA law be derived. Boyle’s Law Pressure and 𝑃1𝑉1 = 𝑃2𝑉2 volume are VISUALIZING THE inversely QUANTUM MECHANICAL proportional when mass and MODEL AND ASSIGNING temperature are QUANTUM NUMBERS TO kept ELECTRONS IN AN ATOM constant. STM 005 (SAS 17) KAAGAPAY SWUDENTS CIRCLE Charles' Law Temperature 𝑉1 𝑉2 = and volume are 𝑇1 𝑇2 QUANTUM MECHANICAL MODEL  MAGNETIC QUANTUM NUMBER, ml allows us to visualize in our minds the three dimensional regions of space around the nucleus of an atom in which there is a good describes the orientation of the orbital in probability of finding electrons space, faster way of determining the orbitals: regions of space number of ml values per sublevel is by there can be two electrons in one orbital using the formula 2/ + 1 maximum Sublevel 𝓁 ml PRINCIPAL QUANTUM NUMBER, n S 0 0 main energy level of an orbital P 1 -1, 0 or +1 total energy of the electron in an atom to determine the maximum number of D 2 -2, -1, 0, 1, electrons that can occupy a main energy 2 2 level, the 2𝑛 rule is followed F 3 -3, -2, -2, 0, 1, 2, 3 AZIMUTHAL QUANTUM NUMBER, 𝓁 represent energy sublevel and can have SPIN QUANTUM NUMBER, ms values beginning with zero and increasing until the integer n-1 is reached electron behaves as though it spins about an axis like a toy top, two orientations are 𝓁 Sublevel Orbital Shape possible for the electron spin: +1/2 and – 1⁄2 (clockwise and counterclockwise spins, 0 S Spherical sometimes represented by an arrow pointing up and down) 1 P Dumbbell 2 D 4 cloverleaf- shaped; 1 dumbbell- shaped with a ring 3 F Too complex to describe RULES GOVERNING THE COMBINATION OF QUANTUM NUMBERS n 𝓁 Kind of sublevel The quantum numbers n, l, and are ml are integers 1 0 1s The principal quantum number, n, cannot be zero (0). Its lowest value is 1. e.g., n= 1, 2, 2 0 2s 3, 4, 5, and so on. ○ Example: 2p5 ; n = 2 3 0 3a The azimuthal quantum number, l, can have a value from 0 to n - 1. The highest value it 3 1 3p can have depends on n. e.g., If n= 6, l can be 0, 1, 2, 3, 4 or 5. 3 2 3d ○ Example: 2p5 ; l = 1  The magnetic quantum number, ml, can be ELECTRONIC CONFIGURATION any integer from -1 to +1 ○ Example: 2p5 ; If l= 1, ml can be -1, 0 or +1 If l= 2, ml, can be -2, -1, 0, +1 summarizes the distribution of electrons or +2 around the atomic orbitals. The spin quantum number, ms, can only be explains an element’s chemical behavior by +1/2 or -1/2. helping determine the valence electrons of an atom. It is often found in most periodic tables and WRITING ELECTRON follows a standard notation. CONFIGURATION OF in writing the electron configuration, it must ATOMS be noted that the total number of electrons that can be accommodated in a shell is STM 005 (SAS 18) KAAGAPAY SWUDENTS CIRCLE based on the principal quantum number (n). ATOMIC ORBITALS can be used to find the probability of location of an electron in a specific region THE THREE GOVERNING FUNDAMENTAL around the nucleus. RULES OF WRITING ELECTRONIC there are four types of orbitals, s, p, d, and f. CONFIGURATIONS ○ the s-orbital is a spherical region of space with high electron density and AUFBAU PRINCIPLE can hold up to a maximum of 2 electrons. this says that the electrons fill the orbitals, ○ the p-orbital is a dumbbell-shaped one at a time, starting with the lowest region of space with high electron energy orbital then proceeding to the one density and can hold a maximum of with higher energy 6 electrons. ○ the d-orbital is a four lobed shaped PAULI EXCLUSION PRINCIPLE region that can hold up to a maximum of 10 electrons. ○ the f-orbital is a multilobed region of this says that no two electrons in the same space with high electron density and atom can have the same set of four can hold a maximum of 14 electrons. quantum numbers applying this rule, the maximum number any s sublevel (with only one orbital) can ORBITAL DIAGRAMS accommodate is two electrons. Each p sublevel has three orbitals and can are used to represent how electrons are therefore accommodate six electrons at arranged in an orbital. most represented by boxes and electrons are the complete filling of the orbitals in the third represented by arrows. main energy level is shown in the following Each block can hold a maximum of two (2) diagram electrons of opposing spins. Take for example the element Hydrogen with electron configuration 1s1 can be represented as:  HUND’S RULE in filling up a set of degenerate orbitals, the orbitals are occupied by one electron at a time with the electrons having the same spin (this is also called parallel spin in contrast to opposite spin). the spinning of electrons generates magnetic spins whose directions depend on the direction of the spin, making it an electric charge in motion. Paramagnetism is the attraction of materials to a magnetic field; it refers to the magnetic state of an atom with one or more unpaired electrons. It has the value of – 1/2. Diamagnetism is the repulsion of materials by magnetic field; these materials are characterized by paired electrons. The reason it repels a magnetic field is because when orbitals are filled with paired electrons, they are spinning in opposite directions, as stated in Pauli’s Exclusion Principle, and as a result, the magnetic field of electrons gets cancelled out, thus there is no magnetic moment. Hence, it has the value of + 1/2 NOBLE GAS NOTATION an abbreviated form of the electronic configuration makes use of the configuration of noble gasses (Group 18) “breathe in, breathe through breathe deep, breathe out” - Taylor Swift