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How Liquids and Solids are formed:
Constant very rapid motion Spaces are larger than the sizes of the molecules itself KE overcomes the forces of atttraction Based on the Kinetic Molecular Theory warm moist air heats the side of the glass, it undergoes condensation and produces water droplets
Water vapor immediately converted to solid, it does not condense. Example: In freezers, frost immediately forms without the need of water if pe is higher than ke then the molecules will be "attached" or fix themselves near to each other if ke is higher than pe, then the molecules will arrange themselves far micro - gamay macro โ dako In gases, KE is greater which explains why particles are far apart from each other Stronger attractions due to touching particles Still randomly move Follows its containers shape Flows slower than gases
intra - one molecule inter - daghan ion - naay charge molecule - wala inter - partially positive / negative chemical - intra or muriatic acid dash - you have covalent bond chlorine is electronegative hydrogen ang ma partially positive mag bond / attract silang duha mag kita para naay attraction broken lines - represent inter molecular
bond - force Bond: covalent bond, ionic bond Nature: covalent compound, ionic compound Ionic โ Metal and Non-Metal Covalent โ both non metals New Sub Topic: Ionic Bonding ionic - metal is written first valence electrons - outermost atomic structure of elements Each side can only accommodate upto two (2) electrons Paired Electrons or 2 electrons on the same side are called lone pairs ang gusto ni maam kay mag tapad ang mga naay partner naay pair: lone pair walay partner: unpaired start with above the symbol, right side and down unahon ug sulat ang unpaired
so f shared their electrons tgt to equally share 8 octet rule: 8 VE dash - covalent bond; dash - 2 valence one/single dash โ single bond (2), double dash โ double bond (4), triple dash โ triple bond (6) Identify the central atom โ highest covalancy no. Covalency number โ the number of atoms that can be shared with other atoms or lets say itโs the number of unpaired electrons/dots C โ 4 unpaired O โ 2 unparied Carbon has greater covalency value (4>2) therefore it is the central atom
just subtract their electronegativity values to determine whether they are polar or non-polar In polar substances, the element with lesser electronegativity value with be positively charged while the larger electronegativity value becomes negatively charged Ex: N โ 3.0 - H โ 2.1 + H is lesser so itโs the positive charged Their difference is 0.9 so its obv polar Polar: 0.5 โ 1. localization - localize siya sa certain area delocalization - pwede mu suroy sa bisag asa in metals, VE are free to move from metal to metal which forms metallic bonds
Forces / Attraction / Interaction ion - naay positive ug negative ion // ionic compound dipole - substance or compound with dipole is polar covalent compound ion dipole forces - ionic compound na nasagol sa polar covalent compound Particularly important in solutions of ionic substances in polar liquids ionic substance in polar liquids mu dissolve such as nacl in polar liquids cations attracted to ions and vice versa
These intermolecular forces weaken the ionic bonds between the sodium and chloride ions so that the sodium chloride dissolves in the water (Figure). Ion-dipole forces in a sodium chloride solution. red line - intermolecular forces of attraction - dipole dipole blue broken lines - repulsion naay partially positive ug negative pole (positive end and negative end) two polar covalents attract among themselves between molecules (polar covalent will rearrange para magduol ang + ug โ ends) polar molecules attract when the positive and negative ends are near weaker than the ion dipole forces neutral - walay charge
Why is it temporary: mu go back sila sa ilang original places kay remember electrons are moving and instances are it will comeback so mawala ang partially positive ug negative electrons are not moving in a constant rate, naay paspas, hinay ug average kung kinsay paspas, mao toy una makabalik so it will go back to its original
London Dispersion Force <Dipole-Dipole < Hydrogen Bonding < Ion - Dipole < Chemical Bond LDF as the weakest, Ion-Dipole as the strongest, but Chemical Bond is much more stronger
