INORGANIC CHEMISTRY
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| have fixed compositions and distinct properties. | Pure substance/substance
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| deals with Matter its composition, properties and its reactions | Inorganic Chemistry
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| anything that occupies space and has mass | Matter
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| quantity of matter that it contains. | mass
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| are substances that cannot be decomposed into simpler substances by chemical means. They are the basic substances out of which all matter is composed | Elements
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| are the substances composed of two or more elements united chemically in definite proportions by mass. They can be decomposed by chemical means into simpler elements. | Compounds
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| composed of two or more kinds of matter where each substance retains its own identity and properties thus it can be separated by physical means | Mixtures
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| have uniform composition throughout | Homogeneous mixtures
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| Compositions of mixtures can vary continuously. | Mixtures
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| are substances whose composition, properties and appearance differ throughout. | Heterogeneous mixtures
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| vinegar, brine, syrup, blood, air, rain, natural gas | Homogeneous mixtures
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| sand in water, chocolate chip ice cream, fruit salad, urine, smog | Heterogeneous mixtures
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| also known as suspension (particularly when they are in liquid form) | Heterogenous mixture
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| 2 or more elements that have been held together by chemical bonds | Compound
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| 1 phase (either solid, liquid, gas) | Homogenous
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| Elements categorized according to three's | Triads
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| Very first attempt of periodic table | Triads
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| color, odor, taste, hardness, physical state, melting point, boiling point, electrical conductivity, malleability, density, solubility, specific gravity. | Physical properties:
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| refer to the characteristics that enable one to distinguish one substance from another. | Properties of Matter
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| rusting metal, burning fuel, milk turning sour | Chemical properties:
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| does not involve a change of one kind of matter into another; no change in the fixed composition of the substance | Physical change
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| involves the transformation or change of one kind of matter into another; it results in the formation of a new substance with different properties | Chemical change
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| ) is organized so scientists can quickly discern the properties of individual elements such as their mass, electron number, electron configuration and their unique chemical properties | The periodic table
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| left side of the table | metals
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| reside on the right side of the table | non-metals
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| How many vertical rows in the periodic table? | 8 vertical rows
IA to VIIIA
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| How many families in each group? | 2
A and B
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| How many horizontal rows? | 7 (7th row is incomplete)
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| The 6 periods end with??? | Inert gases
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| are found among the representative elements in the upper right hand region of the periodic table; halogen family, oxygen family, nitrogen family, etc. | . Non-metal
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| occupy a narrow band between the metal and non-metals like silicon and germanium. | Metalloids
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| group's of 8's (not successful because there were positions in the periodic table wherein 2 elements shared in one position) | Octaves
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| Used the concept of the triads and octaves and devised a way to categorize elements | Modern Periodic Table (Dmitri Mendeleev)
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| Involves transfer of electrons (force of attraction) | Ionic Compound
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| display a wide range of physical properties due to the different types of intermolecular attractions such as different kinds of polar interactions. | covalent compounds
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| Elements and compounds that are electrically neutral | Ions
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| Species with overall positive charges | Cations
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| species with overall negative charges | Anions
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| formed only when electrons move from one atom to another | Ions
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| Compounds formed from positive and negative ions | Ionic compounds
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| Individual atoms can gain or lose electrons | monatomic ions
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| each element that forms cations is... | metal
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| metals tend to form cations, while nonmetals tend to form anions | True
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| Every element in the first column forms a cation with... | charge 1+
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| Every element in the second column forms a cation with charge... | charge 2+
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| Elements in the third to last column almost all form an anion with a... | 2- charge
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| elements living in the second to last column almost all form anions with a ... | 1- charge.
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| Involves sharing of electrons | Covalent compound
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| Atoms can gain a full valence shell (electron) by either sharing electron (covalent bonding) or by transferring electron (ionic bonding) | Octet rule
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| are substances which are made of more than one atom or element | are substances which are made of more than one atom or element
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| What holds these atoms together are strong forces of attraction | chemical bonds
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| Electrons involved in bonding are the outermost electrons in an atom and are called as | valence electrons
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| American chemist who pioneered the relationship between electronic structure and chemical bonds. | G.N. Lewis
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| are often used to represent the valence electrons in atoms and molecules. | Dots
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| consists of the symbol for the element and a dot(s) to represent the outermost electron(s) in the atom. | Lewis Electron-dot Structure
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| the completion of the maximum 8 number of electrons. | Octet rule
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| results from the electrostatic attraction between two oppositely charged ions, the action and the anion | Ionic Bond
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| Atoms that pick up the electrons lost by metals become negative ions or anions. | Ionic Bond
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| arises from the sharing of one or more pairs of electrons between two atoms which have the same tendency to give or pick up electrons | Covalent Bond
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| when a non-metallic element combines with another non-metallic element, electrons are neither gained nor lost by the atoms but are shared. | Okay, true
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| combination of symbols for atoms or ions that are held together chemically. | Chemical formula
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| - is a positive or negative integer that is related to the electronic structure of the atom. | Oxidation Number or Oxidation State
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| o The atom that loses electrons has the positive oxidation number and the atom that gains electrons has the negative oxidation number | True
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| The atom that is more electropositive has the positive oxidation number and the atom that is more electronegative has the negative oxidation number | True
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| compounds formed from the combination of two elements | Binary compounds
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| A number of ionic compounds contain a metal cation and two different elements in the | anion group.
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| These compounds containing three elements are called | ternary compounds.
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| the Latin name of the cation with the lower oxidation state is modified to end in -ous, while the cation with the higher oxidation state will end in –ic | “Classical System”
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| cation with the lower oxidation state is modified to end in | ous
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| cation with the higher oxidation state will end in | ic
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| the English name of the metal is used but the oxidation state is indicated by a Roman numeral enclosed in parentheses | “Stock System”
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| are certain molecular compounds in which hydrogen is combined with a second nonmetallic element | Binary acids
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| refers to the formation of ions from atoms or molecules | Ionization
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| a substance that breaks up into ions in solution | Electrolyte –
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| if a substance completely ionized | Strong electrolyte –
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| if a substance is only partially ionized | Weak electrolyte –
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| one that is only partially ionized | Weak acid or base –
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| one that is completely ionized | Strong acid or base –
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| – type of compound which can act either as acid or base (“amphi” means both kinds) | Amphiprotic or amphoteric
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| a solution which contains a weak acid and its conjugate base or a weak base or conjugate acid. It has a remarkable property of maintaining an almost constant pH even though a strong acid or base is added to the solution | Buffers –
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| high pH of blood | Alkalosis –
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| – low pH of blood | Acidosis
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| weak acids and bases are written in molecular form, and strong acids and bases are written in the form of ions | . Ionic equations –
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| . shows only those ions that actually undergone a chemical change | Net ionic equation –
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| ions which do not undergo any change | Spectator ion –
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| Turns litmus paper to red | Acids
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| Has a sour taste | Acids
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| Neutralizes base | Acids
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| Reacts with active metals to produce hydrogen gas | Acids
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| Has a bitter, biting taste | Base
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| Has a slippery, soapy feeling (due to dissolving a thin layer of the skin) | Base
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| Neutralizes acids | Base
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| Turns litmus paper to blue | Base
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| It is the “battery acid” found in automobile batteries. It is also used as a dehydrating agent (one that has the ability to remove water) | Sulfuric acid
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| The gastric juice in the stomach is 0.1M HCl. It is called Muriatic acid in industry and is used to clean rust and paint from metals and concrete | Hydrochloric acid
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| It is used to make fertilizers and explosives | Nitric acid
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| It is used in dilute form in softdrinks and in detergents and in fertilizers | Phosphoric acid
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| The acid in vinegar is dilute acetic acid | Acetic acid
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| The acid in citrus fruits is citric acid | Citric acid
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| It is found in carbonated drinks | Carbonic acid
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| It is known as lye. It is used in soap manufacture and paper production. It is also used as drain cleaner | Sodium hydroxide
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| Like NaOH, it is a strong base and is used to dissolve grease and hair in clogged drains | Potassium hydroxide
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| As a suspension, it is known as milk of magnesia. In small dosage, it is used as an antacid, but in large amount, it is used as a laxative | Magnesium Hydroxide
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| It is used as an antacid with no dosage restrictions | Aluminum hydroxide
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| It is ammonia dissolved in water. A 2% solution of ammonia is used to revive patients who have fainted, it is used in the production of fertilizers | Ammonium hydroxide
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| used for accurate measurement of pH | pH meter
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| Normal pH range of blood | 7.35 – 7.45
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| pH less than 7.35 | acidosis
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| pH more than 7.45 = alkalosis | alkalosis
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| The reaction between an acid and a base to form a neutral solution | Neutralization
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| It occurs when an equivalent amount of an acid reacts with an equivalent amount of base | Neutralization
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| the point where an acid or base has been added in amounts equivalent to each other | Equivalence point –
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| Used to accomplish equivalence point | Titration
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| the known solution | Standard solution –
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| the point in titration where the indicator used undergoes a color change | End point –
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| Power of hydroxide | pOH
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| if pH = 7 | neutral solution
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| if pH = more than 7 | solution is basic
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| if pH = less than 7 | solution is acidic
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| Power of hydrogen | pH
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| Non-metal oxide | Acid Anhydride
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| non-metal + water = | oxyacid
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| Metal oxide | Basic Anyhydride
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| Acid oxides | Acid Anhydride
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| Basic oxide | Basic Anyhydride
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| metal oxide + water | metal hydroxide (base)
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| Developed as a more convenient way of expressing hydrogen ion concentration | pH and POH concepts
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| increase the concentration of hydrogen ions | Acids
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| decrease the concentration of hydrogen ions (by accepting them) | Bases
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| The acidity or basicity of something, therefore, can be measured by its hydrogen ion concentration. | True
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| invented the pH scale for measuring acidity | Danish biochemist Sören Sörensen
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| pH scale formula | pH = -log [H+]
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| is commonly abbreviated by using square brackets | concentration
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| hydrogen ion concentration | [H+]
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| Substances with a pH between 0 and less than 7 | acids
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| Lower pH means higher hydrogen ion concentration | True
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| Substances with a pH greater than 7 and up to 14 | Bases
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| Higher pH means lower hydrogen ion concentration | True
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| pH= 7 | Neutral
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| Solutions are homogeneous mixtures | True
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| Major component of a solution | Solvent
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| Minor components of a solution | Solute
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| The maximum amount of a substance dissolved in a given volume of solvent is called | Solubility
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| A solution that has reached the maximum solubility | Saturated solution
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| the solute is constantly being dissolved and deposited at an equal rate | equilibrium
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| Substances such as H2, O2, N2, CH4, CCl4 etc. are called | non-polar compounds
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| s H2O, NH3, CH3OH, NO, CO, HCl, H2S, H3P etc. are called | polar compounds
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| liquids that are capable of mixing and forming solutions. | miscible
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| solubility of methyl alcohol and water | miscible
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| liquids that are insoluble in each other | immiscible
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| solubility of oil and water | immiscible
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| Nonpolar compounds tend to be more soluble in nonpolar solvents than in polar solvents | True
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| an increase in temperature results in increased solubility. | True
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| contains a relatively small amount of dissolved solute | dilute solution
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| contains a relatively large amount of solute | concentrated solution
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| expresses the concentration of solution as the percent of solute in a given mass of solution. | Mass percent
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| A final way to express the concentration of a solution is by its | Molality (m)
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| the number of moles of solute per liter of solution. | Molarity (M)
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| is a measure of concentration equal to the gram equivalent weight per liter of solution. | Normality
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| describes the amount of gram equivalent of compound present in the solution | Normality
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| describes the number of moles present in the solution. | Molarity
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| In a chemical reaction atom are neither created nor destroyed. All atoms present in the reactants must also be present in the products. | True
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| is a shorthand expression for a chemical change or reaction. | Chemical equation
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| arrow | indicates the direction of the reaction.
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| The reactants are placed to the left and the products to the right of the arrow | True
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| is placed between reactants and between products when needed. | Plus sign
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| are placed in front of the substances to balance the equation and to indicate the number of units (atoms, molecules, moles, ions) of each substance reacting or being produced. | Coefficient
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| , a delta sign place above the arrow (∆)indicates that __________ is supplied to the reaction | heat
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| The balanced equation therefore obeys the ____________ | law of conservation of mass.
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| A reaction in which two or more substances combine to form a single new substance. | Combination reaction
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| Also called synthesis reactions | Combination reaction
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| A + B ---> AB | Combination reaction
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| are capable of adopting multiple positive charges within their ionic compounds | Transition metals
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| Starts from a single substance and produces more than one substance | Decomposition reaction
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| One substance as a reactant and more than one substance as the products | Decomposition reaction
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| A(+) + BC → B + AC A(-) + BC → C + BA | Single Displacement Reactions
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| Two compounds exchange partners with each other to produce two different compounds | Double Displacement Reactions
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| AB + CD → AD + CB | Double Displacement Reactions
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| solution a system in which one or more substances are _________ or dissolved in another substances | homogeneously mixed
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| least abundant | solute
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| dissolving agent | solvent
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