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Matter and Energy
| Two types of pure substances: | Elements and Compounds |
| The simplest type of pure substance which is composed of only one type of material such as silver, aluminum, or iron: | Element |
| Every element is composed of: | Atoms |
| A type of pure substance that consists of two or more elements always chemically combined in the same proportion: | Compounds |
| In a Mixture, two or more different substances are________ mixed but not ________ combined. | physically; chemically |
| Unlike compounds, the proportions of substances in a mixture are... | Not consistent and can vary. |
| Can compounds be separated into their elements through physical processes? | No |
| Can physical processes be used to separate mixtures? | Yes |
| Why can physical processes be used to separate mixtures? | Because there are no chemical interactions between the components. |
| Type of mixture which is also called a "solution", has a uniform composition throughout, and it's individual components are not visible: | Homogenous mixture |
| Type of mixture which does not have a uniform composition, individual components are visible and appear as two separate regions | Heterogeneous mixture |
| Examples of homogenous mixtures: | Air, seawater, mouthwash |
| Examples of heterogenous mixtures: | Orange juice with pulp, oatmeal raisin cookie, oil and water |
| In a chemistry laboratory, solids are separated from liquids by: | Filtration |
| Physical forms are called: | 3 states of matter |
| 3 states of matter: | Solid, liquid, and gas |
| State of matter that has definite volume and shape, strong attractive forces that hold particles that are close together: | Solid |
| State of matter that has definite volume but NOT definite shape, the particles move in random directions but have strong enough attraction to each other to maintain a definite voume: | Liquid |
| State of matter that has no definite shape, no definite volume, particles are far apart, and have little attraction to each other | Gas |
| Those characteristics that can be observed or measured without affecting the identity of a substance: | Physical properties |
| When matter undergoes a _______ change, it's state, size, or appearance will change, but its composition remains the same: | Physical change |
| ___________ Properties describe the ability of a substance to change into a new substance: | Chemical |
| When a ______ change takes place, the original substance is converted into one or more new substances, which have new physical and chemical properties: | Chemical |
| Physical or Chemical change? Water boils to form water vapor: | Physical |
| Physical or Chemical change? Copper is drawn into thin copper wires: | Physical |
| Physical or Chemical change? Shiny silver metal reacts in air to give a black grainy coating | Chemical |
| Physical or Chemical change? Sugar dissolves in water to form a solution: | Physical |
| Physical or chemical change? A piece of wood burns with a bright flame and produces heat, ashes, carbon dioxide, and water vapor: | Chemical |
| Physical or Chemical change? Paper is cut into tiny pieces of confetti: | Physical |
| Physical or Chemical change? Iron, which is gray and shiny, combines with oxygen to form orange-red rust: | Chemical |
| Science uses what unit of degree to measure temperature? | Celsius |
| Freezing point of water: | 0 degrees C |
| Boiling point of water: | 100 degrees C |
| Human body temp in C | 37.0 degrees C |
| Human body temp in F | 98.6 degrees F |
| How many degrees between boiling and freezing point in Celsius? | 100 C |
| How many degrees between freezing and boiling point in Fahrenheit? | 180 F |
| 1.0 degree C is equal to ____ degree F: | 1.8 degrees F |
| 180 degrees F is equal to ____ degree(s) C: | 100 degrees C |
| Equation to obtain Fahrenheit from Celsius: | TF= 1.8(TC)+32 |
| Celsius temp is multiplied by 1.8 to _______ | Change Celsius to Fahrenheit |
| Then 32 is added to ________ | Adjust the freezing point from Celsius to Fahrenheit |
| Are the values 1.8 and 32 used to determine SFs in the answer? | No, they are exact |
| Equation to obtain degrees C: | TF -32/ 1.8= TC |
| 354 Fahrenheit in C: | 178.8 = 179 |
| 24 degrees Celsius in F: | 75.2 = 75 |
| What is the coldest temp possible? | -273 C (More precisely 273.15 C) |
| 273.15 C in Kelvin (K) | 0 K "Absolute zero" |
| Degrees in Kelvin are called: | Kelvins |
| This temperature scale has no negative temperature values: | Kelvin |
| Freezing point of water in K | 273 K |
| Boiling point of water in K | 373 K |
| difference between boiling and freezing point in Kelvins | 100 kelvins |
| 1 kelvin is equal to 1 degree _____ | Celsius 1K=1C |
| Temperature equation to obtain kelvins from Celsius: | TK=TC+273 |
| How to obtain Kelvins from F | Convert from Kelvin to Celsius first TK=TC+273 then convert your celsius answer to F |
| Energy is defined as: | The ability to do work |
| Two types of energy: | Kinetic and Potential |
| The energy of motion: | Kinetic |
| Any object that is moving has _____ energy: | Kinetic |
| What is potential energy determined by? | The position of an object or the chemical composition of a substance. |
| Example of potential energy: | Boulder on mountain |
| How might that potential energy convert to kinetic energy? | The boulder could roll down the mountain |
| What is the type of energy associated with the motion of particles? | Heat |
| True or false: The particles in an ice cube move very slowly, if you hold the ice cube in your hand, the particles move faster meaning the ice cube now has greater heat or thermal energy: | True |
| The SI unit for energy and work: | Joule (J) |
| The joule is a small amount of energy, so scientists will often use the ______: | Kilojoule (kJ) 1000 joules |
| The calorie is defined as: | exactly 4.184 j |
| Two conversion factors for a calorie into joules | 4.184 j/ 1 cal and 1 cal/4.184 j |
| 1 kilocalorie Kcal is equal to: | 1000 calories |
| 1 kilojoule is equal to: | 1000 joules |
| How to convert joules to calories (sample problem): | j x 1 cal/4.184 j 360 j x 1 cal/4.184 j = 86 cal |
| The nutritional unit Calorie (Cal with a capital C) is equivalent to: | 1000 cal or 1 kcal |
| The energy values for food are ________ | The Kilocalories or Kilojoules obtained from burning 1 g of carbohydrate, fat, or protein. |
| Equation to obtain Kilocalories when given the amount of a nutrient in grams: | Kilocalories = g x Kcal/g |
| Equation to obtain kilojoules when given the amount of a nutrient in grams: | Kilojoules = g x kJ/g |
| How many kcal/g are there in carbohydrates? | 4 kcal/g |
| How many kJ/g are there in carbohydrates? | 17kJ/g |
| How many kcal/g are there in fat? | 9kcal/g |
| How many kJ/g are there in fat? | 38 kJ/g |
| How many kcal/g are there in protein? | 4 kcal/g |
| How many kJ/g are there in protein? | 17 kJ/g |
| Equation to obtain percentage of fat in one serving of snack crackers: | Percentage of fat = energy from fat/ total energy x 100 |
| What is specific heat? | The specific heat (SH) of a substance is defined as the amount of heat needed to raise the temperature of exactly 1 g of a substance by exactly 1 degree Celsius |
| How is the temperature change written? | ΔT |
| What does Δ mean? | "Change in" |
| Specific heat equation: | SH = cal (or J)/g x degree celsius (ΔT) |
| True or false? The specific heat expression can be rearranged to solve for heat as long as you know the specific heat: | True |
| Heat equation using calories: | Heat = m x ΔT x SH = Cal = g x degree C x cal/g x degree celsius |
| Heat equation for joules: | J= g x Degree C x J/ g x degree Celsius |
| Specific heat of water: | 1 cal/g degree C = 4.184 j/ g degree C |
| When heat is added to a solid, do the particles move faster or slower? | Faster |
| At a temperature called:_____________, The particles of a solid gain sufficient energy to overcome the attractive forces that hold them together: | Melting Point (mp) |
| Matter changing from a solid to a liquid is called_____ | Melting |
| A liquid changes to a solid at its ______: | Freezing point |
| True or false: The melting point (mp) and freezing point (fp) of a substance are the same temperature: | True |
| During melting, the _______ is the energy that must be added to convert exactly 1 g of solid to liquid at the melting point: | Heat of fusion |
| How many cal or J are needed to melt exactly 1 g of ice at its melting point (0 degrees C? | 80. cal (334 j) |
| Equation to calculate heat needed to melt or freeze water: | heat = mass x heat of fusion cal= g x 80. cal/g J= g x 334 J/g |
| In a process called ______ the particles on the surface of a solid change directly to a gas, without going through the liquid state: | Sublimation |
| ________ Is taking place as particles with sufficient energy escape from the liquid surface and enter the gas phase: | Evaporation |
| reverse of evaporation, water vapor is converted back to liquid as the water particles lose kinetic energy and slow down: | Condensation |
| Condensation occurs at the same temperature as: | Boiling point |
| The _________ is the energy that must be added to convert exactly 1 g of liquid to gas at its boiling point: | Heat of vaporization |
| For water, how many cal are needed to convert 1 g of water to vapor at 100 degrees C? | 540 cal |
| For water how many J are needed to convert 1 g of water to vapor at 100 degrees C? | 2260 J |
| Write the two conversion factors for the "heat of condensation" and the "heat of vaporization": | 540 cal/1 g H2O and 2260 J /1 g H2O ( and vice versa) |
| Write equation for calculating heat to condense (or boil) water: | Heat = mass x heat of vaporization cal = g x 540 cal/ g J= 2260 J/ g |
| ______ Equation would be used to calculate how much energy/heat needs to be added or removed to melt or heat water: | Heat of fusion |
| ________ equation would be used to determine how much heat is added or released when liquid turns to vapor or vapor to liquid: | Heat of vaporization/heat of condensation |
Created by:
Lilielena
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