AP Chemistry : Chapter 1 Flashcards
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| 10635850873 | Chemistry | study of matter (such as the changes it undergoes, properties, and behavior) | 0 | |
| 10635850874 | Matter | • physical material of universe • has mass and occupies space | 1 | |
| 10635850875 | Property | any characteristic that allows recognition to a particular type of matter and distinguishes it from other types | 2 | |
| 10635850876 | Elements | substances that compose matter | 3 | |
| 10635850877 | Atoms | small building blocks of matter | 4 | |
| 10635850878 | Molecules | 2 or more atoms are joined in specific shapes | 5 | |
| 10635850879 | Chemistry is used for...(4) | • energy • biochemistry • technology • medicine. | 6 | |
| 10635850880 | 3 things chemists do: | • Make new types of matter: materials, substances, or combinations of substances with desired properties • Measure the properties of matter • Develop models that explain and/or predict the properties of matter | 7 | |
| 10635850881 | 2 ways Matter is characterized by: | • Its physical state (States of matter) • its composition | 8 | |
| 10635850882 | 3 states of matter | • gas • liquid • solid | 9 | |
| 10635850883 | gas | Molecules are far apart, moving at high speeds, colliding with each other and walls. Increasing compression reduces the amount of space and makes them collide more frequently; no fixed volume or shape ; uniformly fills its container | 10 | |
| 10635850884 | liquid | molecules packed closely together; move rapidly making them slide over each other; has a distinct volume dependent of its container ; assumes the shape of the portion of the container it occupies | 11 | |
| 10635850885 | solid | molecules are held tightly together in definite arrangements; has a definite shape and a definite volume; Uniformly fills | 12 | |
| 10635850886 | Types of composition(3) | • Element • Compound • Mixture | 13 | |
| 10635850887 | What is similar/different about liquids and solids? | The distance between molecules but they differ in how freely they are. | 14 | |
| 10635850888 | Pure substance | matter that has distinct properties and a composition that does not vary from sample to sample. | 15 | |
| 10635850889 | 2 types of pure substances: | • Elements • Compounds | 16 | |
| 10635850890 | Elements | • substances that cannot be decomposed into simpler substances • Contain only one atom | 17 | |
| 10635850891 | Compounds | • substances composed of 2 or more elements • contain 2 different atoms | 18 | |
| 10635850892 | Mixtures | combinations of two or more substances in which each substance retains its chemical identity. Its composition can vary. | 19 | |
| 10635850893 | 2 types of mixtures | • heterogenous mixtures • homogenous mixtures | 20 | |
| 10635850894 | Heterogenous mixtures | mixtures do not have same composition, properties, and appearance throughout | 21 | |
| 10635850895 | Homogenous mixtures | mixtures that are uniform throughout | 22 | |
| 10635850896 | Another name for homogenous mixtures | solutions | 23 | |
| 10635850897 | The law of constant composition (law of definite proportions) | observation that the elemental composition of a compound is always the same | 24 | |
| 10635850898 | 2 types of properties of matter: | • physical properties • chemical properties | 25 | |
| 10635850899 | Physical properties | observed without changing identity and composition of substance. | 26 | |
| 10635850900 | examples of physical properties: | • color • order • density • boiling point • melting point • hardness | 27 | |
| 10635850901 | Chemical properties | describe way a substance may change(react) to form other substances | 28 | |
| 10635850902 | example of chemical property : | • flammability | 29 | |
| 10635850903 | Intensive properties | do not depend on amount of examined sample and can identify substances | 30 | |
| 10635850904 | Examples of intensive properties: | • temperature • melting point | 31 | |
| 10635850905 | Extensive properties | depend on amount of sample | 32 | |
| 10635850906 | Examples of extensive properties: | • mass • volume | 33 | |
| 10635850907 | 2 changes substances undergo | • physical change • chemical change | 34 | |
| 10635850908 | Physical change | substance changes its physical appearance but not its composition | 35 | |
| 10635850909 | Example of a physical change: | • All changes of state | 36 | |
| 10635850910 | Chemical change (chemical reaction) | substance is transformed into a chemically different substance | 37 | |
| 10635850911 | The separation of mixtures takes advantage of... | differences in properties | 38 | |
| 10635850912 | 3 ways to separate compounds | • filtration • distillation • chromatography | 39 | |
| 10635850913 | Distillation | process used in homogenous mixtures to separate its components and is dependent on different abilities of substances to for gases. | 40 | |
| 10635850914 | Metric system | units used for scientific measurements | 41 | |
| 10635850915 | The scientific method(4) | Observations Question Hypothesis Theory | 42 | |
| 10635850916 | Scientific Law | constant repeated behavior that nature does under different conditions | 43 | |
| 10635850917 | Law of conservation of mass | In a chemical reaction there is no change in the total mass of materials reacting when compared to those that have formed. | 44 | |
| 10635850918 | Mass | measure of amount of material in an object | 45 | |
| 10635850919 | Temperature | • measure of hotness/coldness of an object • a physical property that determines direction of heat flow (flows spontaneously from substance of high heat to one with lower temp.) | 46 | |
| 10635850920 | • Freezing point: • Boiling point: | • Freezing point: 0 ° C (32 ° F) • Boiling point: 100 ° C (212 ° F) at sea level | 47 | |
| 10635850921 | Weight | the force that is exerted on the mass of an object by gravity | 48 | |
| 10635850922 | Zero on Kelvin scale is also known as | absolute zero | 49 | |
| 10635850955 | Formula for Fahrenheit |  | 50 | |
| 10635850923 | Derived unit | obtained by multiplication or division of one or more of the base units | 51 | |
| 10635850924 | Volume of cube = | length³ | 52 | |
| 10635850925 | 1 liter = | Dm³ (cubic decimeter) | 53 | |
| 10635850926 | 1 mL = | 1 cm³ | 54 | |
| 10635850927 | Density | The amount of mass in a unit volume of a substance | 55 | |
| 10635850928 | Density = ___________ ÷ _____________ | mass / volume | 56 | |
| 10635850929 | What is density dependent on? | temperature | 57 | |
| 10635850930 | If no temperature is reported, we assume what temperature? | 25 °C | 58 | |
| 10635850931 | Two kinds of numbers encountered in scientific work: | • exact numbers • inexact numbers | 59 | |
| 10635850932 | exact numbers | those whose values are known exactly | 60 | |
| 10635850933 | inexact numbers | those whose values have some uncertainty | 61 | |
| 10635850934 | Numbers obtained by measurements are what type of numbers? Why? | • inexact numbers • Due to equipment error and human error | 62 | |
| 10635850935 | Precision | measure of how closely individual measurements agree with one another | 63 | |
| 10635850936 | Accuracy | Refers to how close individual measurement agree with the correct/"true" value. | 64 | |
| 10635850937 | Standard deviation | reflects how much the individual measurements differ from the averages | 65 | |
| 10635850938 | Standard deviation is the ____________ of measurements | precision | 66 | |
| 10635850939 | small sd = | nearly same values | 67 | |
| 10635850940 | There is always some uncertainty in the _______ digit reported for any measured quantity | last | 68 | |
| 10635850941 | Significant figures | All of the digits of a measured quantity, including the uncertain one | 69 | |
| 10635850942 | The more sig figs, the greater the ____________ for the measurement | accuracy | 70 | |
| 10635850943 | Rules for significant figures: | • All nonzero digits are significant • Zeros between nonzero digits are always significant • Zeros at the boggling of a number are never significant • Zeros at the end of a number are significant if there is a decimal point | 71 | |
| 10635850944 | Rules for sig figs in Addition and subtraction | result has same number of decimal places as the measurement with the least decimal places | 72 | |
| 10635850945 | Rules for sig figs in Multiplication and division | result contains same number of sig. figs. as the measurement with the fewest sig. figs. | 73 | |
| 10635850946 | For calculations with more than one step | Do nott round in between steps, just round at the end | 74 | |
| 10635850947 | Dimensional Analysis | units are multiplied together or divided into each other along with the numerical values | 75 | |
| 10635850948 | 1 in. = _____ cm. | 2.54 cm. | 76 | |
| 10635850949 | 1 lb. = _____ g. | 453.6 g. | 77 | |
| 10635850950 | 1 mile = _____ km. | 1.6093 km. | 78 | |
| 10635850951 | 1.00 g. water = _____ mL. water | 1 mL water | 79 | |
| 10635850952 | 1 L = _____ qt. | 1.057 qt. | 80 | |
| 10635850953 | 1 gal. = _____ qt.. | 4 qt. | 81 |