![]() ![]() The elements on the periodic table are listed in order of ascending atomic number. If blood pH rises to 7.8, alkalosis results.\), while one may view a more extensive periodic table from another source. What happens if the pH of blood is changed? If blood pH drops to 7, acidosis results. Buffers keep the pH within normal limits because they are chemicals that take up excess H ions or OH- ions. Buffers, among other things, keep the pH of blood around 7.4. A buffer is a chemical or combination of chemicals that keeps pH within normal limits. = 10-pOH or antilog (-pOH) Analyze how buffers prevent large pH changes in solutions. Determine pH from H or OH- concentration. The scale ranges from 0 to 14, 0 being extremely acidic and 14 being very basic. If it has a -2 charge, there must be two more electrons than protons. If you are told an atom has a 1 charge, that means there is one less electron than protons. Ions are atoms don't have the same number of electrons as protons. Anything below 7 is acidic and anything above is basic. For protons, the number always equals the atomic number of the element. Acidic:Īmmonia The pH scale On the pH scale, 7 is neutral (like water, sugar, and table salt). Identify some common acidic and basic substances. Ice is therefore less dense than liquid water and floats on it. This means that water expands as it reaches 0C and freezes. At temperatures below 4C only vibrational movement occurs and hydrogen bonding becomes more rigid but also more open. Frozen Water (Ice) is Less Dense Than Liquid Water -water becomes most dense at 4 C but the molecules are still moving around. Adhesion is the ability of water molecules to cling to other polar surfaces as a result of water's polarity.Ħ. Because of this, water exists as a liquid in the conditions present at the Earth's surface. Cohesive and Adhesive-Cohesion is the ability of water molecules to cling to each other due to hydrogen bonding. it dissolves a great number of substancesĥ. Solvent-due to its polarity, water facilitates chemical reactions both inside and outside living systems. A High Heat of Evaporation -hydrogen bonds must be broken before water can boil so converting 1 gram of the hottest water to gas takes 540 calories.Ĥ. ![]() because of the many hydrogen bonds that link water molecules, water can absorb heat without a great change in temperature.ģ. A High Heat Capacity -water requires a calorie of energy to raise the temperature one degree Celsius, other covalently bonded liquids require half this. responsible for water being a liquid at normal temperaturesĢ. Hydrogen bonding -water molecules cling together. solvent substance that dissolves solution complete mixture solute substance that is dissolved List and analyze the properties of water. This attraction causes the slightly positive and negative ions to dissociate. The negative ends of water molecules are attracted to slightly positive atoms and the positive ends of water molecules are attracted to slightly negative atoms. Hydrogen Bonding: (especially water, but not unique to it) more easily broken than other bonds, the attraction of a slightly positive hydrogen to a slightly negative atom in the vicinity, a polar covalent bond Polar when electrons are not shared equally Describe how water associates with other molecules in solution. ![]() If one atom is better able to attract electrons than the other atom, it is more electronegative.ģ. <-nonpolar and polar covalent bonds→ Nonpolar- when the sharing of electrons between two atoms is equal. Covalent Bonds (joint sharing): Bonding when two atoms share electrons in such a way that each atom has an octet of electrons on the outer shell. Ionic Bonding (donation): Electron transfer that causes a charge imbalance in each atom (thus the name "ionic" for ion) Held together by a strong attraction between negatively and positively charged ions.Ģ. Elements can be combined to form molecules and compounds through different bonds.ġ. Describe how elements are combined into molecules and compounds. What makes up the inside of an atom? Most of an atom is empty space. If an atom could be drawn the size of a football field, the nucleus would be like a gum-ball in the center and the electrons tiny specks whirling around the upper stands. The concept has changed greatly from that time. John Dalton developed the atomic theory, which stated that elements consisted of tiny particles called atoms. Valence shell outermost shell Determine how electrons are configured around a nucleus. ![]()
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