| A | B |
|---|
| What are the building blocks of all matter? | atoms |
| The nucleus of an atom is made up of ____ and ____ | protons and neutrons |
| Electrons have a ___ charge | negative |
| Protons have a ___ charge | positive |
| Neutrons have a ___ charge | neutral (no) charge |
| Which type of particle orbits the nucleus? | electrons |
| Positive charges are attracted to ____ charges | negative |
| Positive charges are repelled by ____ charges. | positive |
| Negative charges are repelled by ____ charges | negative |
| An electron would be attracted to a _____ | proton |
| The center region of an atom is called a(n) ____. | atomic nucleus |
| Each element is different because they have a different number of ____. | protons |
| All of the elements are listed in the ____. | periodic table |
| The ____ is equal to the number of protons in an atom. | atomic number |
| The number of protons + the number of neutrons is equal to the ____ | mass number |
| The mass number is equal to the | number of protons and neutrons |
| The atomic number is equal to the number of ____ in an atom | protons |
| The number below the chemical symbol on the periodic table that usually has a few decimal places is known as the ____. | average atomic mass |
| If an element has a mass # of 23 and an atomic # of 11, how many protons will it have? Neutrons? | 11 protons and 12 neutrons |
| Two or more different elements bond together to form ____. | compounds |
| A compound held together by covalent bonds is called a(n) ___. | molecule |
| Atoms or molecules that become charged because they gain or lose electrons are called ___. | ions |
| A negatively charged ion would be ____ by another negatively charged ion. | repelled |
| A positively charged ion would be ____ by another positively charged ion. | repelled |
| A negatively charged ion would be ___ by a positively charged ion. | attracted |
| A liquid that has a uniform mixture of two or more substances is know as a(n) ___. | solution |
| In a glass of salt water, the ___ would be the solvent. | water |
| In a glass of salt water, the ___ would be the solute. | salt |
| In a solution of sugar and water, the sugar would be the ___. | solute |
| In a solution of sugar and water, the water would be the _____. | solvent |
| Acids have a pH that is ____ seven. | below |
| Bases have a pH that is ___ seven. | above |
| Distilled water has a pH of ___. | seven |
| A liquid with a pH of 1 would be described as being ___ than a liquid with a pH of 5. | more acidic |
| A liquid with a pH of 6 would be described as being ___ than a liquid with a pH of 2 | less acidic |
| A liquid with a pH of 8 would be described as being ___ than a liquid with a pH of 14. | less basic |
| A liquid with a pH of 13 would be described as being ___ than a liquid with a pH of 7.8. | more basic |
| As temperature ____, particles move faster and faster | increases |
| As temperature ____ particles move slower and slower. | decreases |
| Increasing the ___ or ___ of the reactants will cause a reaction to speed up. | temperature, concentration |
| Matter is _____. | Anything that takes up space and has mass. |
| _____ is anything that takes up space and has mass. | Matter |
| A(n) ______ is a substance that cannot be broken down to other substances by chemical reactions. | element |
| Two types of compounds are ____ and ____. | molecules and ionic compounds. |
| A compound in which atoms are joined together by ionic bonds is called a(n) ___. | ionic compound |
| Give an example of a molecule that is not a compound. | Any diatomic molecule, like O2, or H2, or N2, is a molecule because the two atoms are joined by covalent bonds, but is not a compound because they aren't made of two or move DIFFERENT elements. Diatomic molecules are called pure elements. |
| Which 4 elements make up 96% of living matter? | Carbon, Hydrogen, Oxygen, and Nitrogen |
| Elements that are only required by organisms in minute quantities are called _____. | trace elements |
| A deficiency of the trace element ____ in the diet can lead to an enlargement of the thyroid. This enlargement is called a _____. | iodine, goiter (the enlarged part of the neck in the picture below is the goiter),  |
| A(n) ___ is the smallest unit of matter that still retains the properties of an element. | atom |
| The tiny bits of matter that make up an atom are called ___. | subatomic particles |
| Protons and neutrons each have a mass of 1 _____ (a.k.a. _____) | dalton, atomic mass unit (amu) |
| Isotopes of a certain element have the same number of ____ but differ in the number of _____. | protons, neutrons |
| Elements that differ from each other because of the number neutrons, but not protons, are called ____. | isotopes |
| Scientists use _____ to label certain chemical substances, creating tracers that can be used to follow a metabolic process or locate the substance within an organism. | radioactive isotopes |
| _____ is defined as the capacity to cause change. | Energy |
| ____ is the energy that matter possesses due to its location or structure. | Potential energy |
| Matter has a natural tendency to move to the ____ possible state of potential energy. | lowest |
| Electrons gain potential energy when they move ____ from the nucleus. | away |
| When an electron falls back toward the nucleus, energy is ___. | released (or lost) |
| The different states of potential energy that electrons have in an atom are called _____ and are represented by ____. | energy levels, electron shells |
| When electrons lose energy (by falling back toward the nucleus), the lost energy is usually released to the environment in the form of ___. | heat |
| The first electron shell of an atom can hold no more than ___ electrons. | 2 |
| The second electron shell of an atom can hold no more than ___ electrons. | 8 |
| The chemical behavior of an element depends mostly on ____. | the number of electrons in its outermost shell |
| Electrons in the outermost shell of an atom are called ____. | valence electrons |
| The outermost shell of an atom is called the ___. | valence shell |
| An atom with a full valence shell of electrons is chemically _____ (a.k.a. _____) | unreactive, inert |
| The three-dimensional space where an electron can be found 90% of the time is called a(n) ___. | orbital |
| A maximum of ___ electrons can be found in any one orbital. | 2 (Don't get orbitals mixed up with shells or energy levels. For instance, the second energy level has 4 orbitals. One s-orbital and three p-orbitals) |
| Spherical orbitals are called ____ and there is/are ____ of these at each energy level. | s-orbital, one,  |
| Dumbbell shaped orbitals are called ____ and there is/are ____ of these at each energy level. | p-orbital, 3 at each energy level except the first which has none, |
| The only type of bond that is categorized as being strong is a(n) _____ bond. | covalent |
| In _____ bonds, pairs of electrons are shared between two or more atoms. | covalent |
| Single covalent bonds share ___ pair(s) of electrons. | one pair (two electrons total) |
| Double covalent bonds share ___ pair(s) of electrons. | two pairs (4 electrons total) |
| Triple covalent bonds share ___ pair(s) of electrons. | three pairs (6 electrons total) |
| Write the molecular formula for a molecule of oxygen. | .,  |
| Write the structural formula for a molecule of oxygen. | .,  |
| Draw the electron shell diagram for a molecule of oxygen. | .,  |
| The number of covalent bonds that an atom can form is called its _______ or ________ and is usually equal to the number of ______ in the atoms outermost shell. | bonding capacity or valence, usually equal to the number of unpaired electrons in the atoms outermost (valence) shell. |
| The attraction of a particular kind of atom for the electrons of a covalent bond is called its ___. | electronegativity |
| The more ____ an atom is, the more strongly it pulls shared electrons toward itself. | electronegative |
| The _____ electronegative an atom is, the more strongly it pulls shared electrons toward itself. | more |
| Bonds in which the electrons between two atoms are shared about equally (because both atoms have similar electronegativities) are called _____. | nonpolar covalent bonds |
| Bonds in which the electrons between two atoms are not SHARED equally (because one atom has a significantly higher electronegativity) are called _____. | polar covalent bond |
| Bonds in which electrons aren't shared at all (because one atom has a MUCH higher electronegativity than the other) are called ______. | ionic bonds |
| A charged atom, (or molecule) is called a(n) ___. | ion |
| Positively charged ions are called ____. | cations |
| Negatively charged ions are called ____. | anions |
| Compounds formed by ionic bonds are called ____ . | ionic compounds |
| The most important characteristic about a biological molecule is its ____. | shape |
| The s-orbital and 3 p-orbitals hybidize to form the shape of a ______. This is important because it helps explain why bonds coming off many atoms go off at the angles found in this shape. | tetrahedron,  |
In the chemical reaction picture below, the molecules on the left side of arrow are called the ____ while the molecules on the right side of the arrow are called the ____.,  | reactants, products (notice how there are the same number of each type of atom on both sides of this balanced chemical reaction),  |
The picture below shows the formation of a(n) _____ bond.,  | ionic, |
| A chemical reaction in which arrows are pointing both ways is said to be ____. | reversible |
| In a reversible reaction, when the forward and reverse reactions are happening at the same rate, _____ is achieved. | chemical equilibrium |
| True or false: When a reversible chemical reaction reaches equilibrium, the reactants and products are equal in concentration. | False. All it means is that the concentration of reactants and products has stabilized at some fixed ratio. For example, pure distilled water occasionally breaks down into a hydrogen ion and a hydroxide ion. The hydroxide ions almost instantaneously react with the hydrogen ions to reform water. At any one moment, at equilibrium, there are 554 million times more water molecules than there are hydrogen or hydroxide ions in a solution of distilled water (at 25 Celsius) |
| Name 3 types of weak bonds in order from strongest to weakest. | (strongest) ionic, hydrogen, London Dispersion forces (weakest): Your book calls London Dispersion forces Van der Waals forces, but Van der Waals forces are actually any type of intermolecular force, including hydrogen bonds. |
| Hydrogen bonds usually form between hydrogen atoms involved in a polar covalent bond and _____ or _____ atoms in another molecule. | oxygen, nitrogen |
| A weak attraction between hydrogen in one molecule and either an oxygen or nitrogen atom in another molecule is called a(n) _____. | hydrogen bond |
| A very weak bond that can form between a non-polar region of a molecule and another molecule (as long as the molecules are very close together) is called a(n) ____. | London Dispersion Force (Your book calles London Dispersion forces Van der Waals forces, but Van der Waals forces are actually any type of intermolecular force, including hydrogen bonds.) |
| London Dispersion Forces are very weak attractions between two molecules and involve _____ regions. | non-polar |
| The type of bond that allows certain geckos to walk up walls is called a(n) _____ | London Dispersion Force |
______ bonds allow the endorphin receptors to temporarily bond to morphine or your bodies own natural endorphins because the shapes of the molecules are ____.,  | weak, complementary, |
| Because oxygen is more electronegative than hydrogen, the electrons of the polar covalent bonds spend more time closer to the _______ atom, giving it a partial _____ charge. | oxygen, negative |
| The hydrogen atoms in a water molecule have a _____ _____ charge. | partial positive charge |
| Molecules in which opposite ends of the molecule have opposite charges are called ______. | polar molecules |
| The extraordinary qualities of water are _______ properties resulting from the ______ bonding that orders molecules into a higher level of structural organization. | emergent, hydrogen |
Why is it unlikely that two neighboring water molecules would arrange themselves like the ones shown below?,  | The hydrogen ends of each water molecule both have a partial positive charge, and therefore would repel each other, making it unlikely that they would be arranged like the picture below shows., |
| The fact that water molecules are attracted to each other is an example of ____. | cohesion |
| The ability to pour water into a glass past the top of the glass, water forming drops that stick together, and waterbugs not falling through the surface of a pond can be explained by the phenomenon of _____. | cohesion |
| The attraction of water molecules to the surfaces of some materials is called _____. | adhesion |
The meniscus observed in a graduated cylinder full of water is caused by the ____ of water to the molecules that make up the glass in the cylinder.,  | adhesion, |
| What are the four emergent properties of water that contribute to Earth's fitness for life? | 1) Cohesion 2) Ability to moderate temperature 3) Insulation of bodies of water by floating ice 4) Waters ability as a solvent |
| The energy of motion is called ____. | kinetic energy |
| The total amount of kinetic energy due to molecular motion in a body of matter is described as the ___ within that body of matter. | heat |
| The average kinetic energy of the molecules in a body of matter is measured as _____. | temperature |
| Pure water freezes at ___ Celsius and boils at ___ Celsius. | 0, 100 |
| A calorie is the amount of heat energy needed to raise the temperature of ____ g of water by ____ degree Celsius. | 1,1 |
| The "calories" on food packages are actually _____. | kilocalories (1000 calories = 1 kilocalorie) |
| A joule (J) is a measure of ____. | energy |
| The ____ of a substance is defined as the amount of heat (energy) that must be absorbed or lost by a substance to change its temperature by 1 degree Celsius. | specific heat (In the graph below, it shows that the specific heat is 1cal/C for the liquid phase of water. This is represented by the gentle upwardly sloping part of the graph between 0 and 100C),  |
| Compared with most other substances, water has an unusually high ____ which explains why it can store a lot of energy and it takes a lot of energy to change its temperature. | specific heat |
| Why doesn't it get really cold or really hot when you are out at sea? | The high specific heat of water allows it to absorb a lot of heat from the air without increasing its own temperature too much. When cold air blows over the ocean, the large amount of heat (not to be confused with temperature) can be transferred to the air. Since air has a much lower specific heat, it will warm up easily. In places like the Bering Sea of Alaska, the ocean water keeps the air from getting too much below 20 degrees Fahrenheit even in the middle of winter. In summer, it keeps the air from getting too much above 55 degrees F. |
| The transformation from a liquid to a gas is called ____ or ____. | evaporation or vaporization (boiling is the temperature at which the average molecule has enough energy to overcome the attractions that hold molecules together as a liquid. Therefore, the molecules vaporize quite quickly once the boiling point has been reached) |
| The _____ is the amount of heat needed to convert 1 gram of a substance already at it's boiling point from a liquid to a gas. | heat of vaporization (Even though a liquid has reached it's boiling point, more energy is needed to break the intermolecular bonds between the molecules so they can separate. In the case of water with it's relatively strong hydrogen bonds giving water molecules strong cohesion, it takes a relatively high heat of vaporization to change liquid into gas. Likewise, when water condenses, a lot of heat is quickly released as those hydrogen bonds reform. That's why you don't want to keep your hand over a steaming pot of water long enough for the water vapor to condense on your skin.), |
| 1 calorie of energy must be absorbed by water at 99 Celsius to reach 100 Celsius. How many calories must water at 100 Celsius absorb to reach 101 Celsius? | If you answered 1 calorie, you are wrong. To reach 101 Celsius, water must first be converted from a liquid to a gas. This involves the breaking of hydrogen bonds that hold the water molecules together as a liquid. To break all the hydrogen bonds requires much more energy than it does to simply get the molecules in liquid water to move faster by an average of 1 degree Celsius. This energy requirement is called the heat of vaporization, which is quite high for water compared to most liquids., |
| Water helps moderate Earth's temperature by _____ a lot of heat to become water vapor at the equator and then moving toward the poles to ____ that heat as it _____. | absorbing, release, condenses |
| The _____ of water from humans and other organisms helps keep them cool. | evaporation |
| Water reaches its greatest density at ___ degrees Celsius. | 4,  |
| In a lake during winter, where all the water is close to freezing, where would you find the warmest water? | At the bottom, because water that is colder than 4 Celsius is less dense than water at 4 Celsius. All the water in a lake in winter will be less than 4 Celsius, so the coldest water, being the least dense, rises to the surface., |
| In a lake during summer, where would you find the warmest water? | Close to the surface. As long as water is more than 4 Celsius, it behaves like most substances, becoming less dense (and floating) as temperature increases., |
| If ice didn't float, lakes and oceans would ______. | eventually freeze solid because ice would sink, exposing liquid water to cold winter temperatures instead of insulating it from the cold temperatures. |
| An ______ solution is a solution in which water is the solvent. | aqueous |
| The type of substances that dissolve best in water are ____. | ionic substances and polar covalent substances |
| Any substance that is attracted to water is said to be ____. | hydrophilic (hydro = water, philic = loving) |
| Any substance that is repelled by water is said to be ____. | hydrophobic (hydro = water, phobic = fearing) |
| A mixture of liquid with a substance that remains suspended in the liquid (instead of dissolving) is called a(n) ____. | colloid |
| 1 mole of a substance is equal to ____ particles of that substance | 6.02 X 10 ^23 (6.02 times ten to the twenty third power) |
| How do you figure out the molecular mass of a molecule? | Add up the atomic masses of every atom in the molecule {Your answer will be in Daltons (or amu's). To figure out the mass of one mole of that molecule, just change the unit to grams) |
| How would you go about making a 2 molar solution of glucose? | Add 2 moles of glucose to about 1/2 a liter of water. Stir it until it is completely dissolved, then add more water until you have exactly 1 liter of solution. Molarity is defined as the number of moles per liter of solution. Therefore, you would need to figure out the mass of one mole of glucose (by adding up the atomic masses of 6 carbon, 12 hydrogen, and 6 oxygen atoms), multiplying that by two to get 2 moles, massing it out on a balance and dissolving it in water as described in the first sentence. |
Which type of bond is represented by the dotted line? By the straight line inside the water molecule?,  | Dotted lines = hydrogen bonds, straight lines = covalent bonds, |
The picture below shows water dissociating into ___ and ___ ions.,  | hydronium and hydroxide ions,  |
| If the concentration of hydrogen (hydronium) ions in a solution is higher than the concentration of hydroxide ions, the solution will be ____. | acidic |
The substance shown below is a(n) ____ and an increase in its concentration will cause a(n) ___ in pH.,  | hydrogen ion, drop in pH (to become more acidic), |
The substance shown below is a(n) ____ and an increase in its concentration will cause a(n) ___ in pH.,  | hydronium ion, drop in pH (to become more acidic), |
The substance shown below is a(n) ____ and an increase in its concentration will cause a(n) ___ in pH.,  | hydroxide ion, increase in pH (to become more basic) |
.,  | strong acids,  |
.,  | strong bases |
.,  | weak acid, |
.,  | weak bases, |
| The pH scale is kind of like the richter scale (for earthquakes) in that a change of one (such as going from pH 4 to pH 3) represents a ___-fold change. | 10-fold change (for example, pH 3 is 10 times more acidic than pH 4) |
| _____ are substances that minimize (or dampen) changes in pH. | Buffers |
| _____ work by accepting hydrogen ions from the solution when they are in excess and donating hydrogen ions to the solution when they have been depleted. They usually contain a _____ and its corresponding ____. | Buffers, weak acid, base |
| Acid precipitation refers to rain, snow, or fog with a pH less than ____. | 5.6 (which is the normal pH of rain due to carbon dioxide from the atmosphere mixing with on its way down to form carbonic acid) |
| Acidic rain is better at dissolving ______ like aluminum in the soil and dissolving and washing away calcium and magnesium ions which are _______for plant growth. All of these effects are bad for the environment. | toxic metals, essential nutrients |
| The binding together of like molecules, often by hydrogen bonds, is called ____. | cohesion |
| Weak attractions between molecules, or parts of molecules, that are brought about by localized charge fluctuations are called ____. | Van der Waals interactions |
| A common measure of solute concentration, referring to the number of moles of solute per liter of solution is called ___. | molarity |
The sphere of water molecules around each dissolved ion is called a(n) ___.,  | hydration sphere, |
| The property of a liquid whereby the surface becomes cooler during evaporation, due to the loss of highly kinetic molecules to the gaseous state, is called ____. | evaporative cooling |
| A substance that reduces the hydrogen ion concentration of a solution is called a(n) ___. | base |
| A water molecule that has lost a proton is called a(n) ____. | hydroxide ion (remember, a proton is the same thing as a hydrogen ion because hydrogen normally has one proton, 1 electron and no neutrons, so when it becomes a positively charged ion by losing an electron, all that is left is a single proton) |
| The attraction between DIFFERENT kinds of molecules is called ____. | adhesion |
| A measure of how difficult it is to break or stretch the surface of a liquid is called ___. | surface tension |
| The pH of a solution with a hydronium ion concentration of 1 X 10^-7 (one times 10 to the negative seven) moles per liter is _____. | 7 (remember, pH is equal to the negative log of the hydronium ion concentration) |
| The pH of a solution with a hydronium ion concentration of 1 X 10^-3 (one times 10 to the negative three) moles per liter is _____. | 3 (remember, pH is equal to the negative log of the hydronium ion concentration) |
| The pH of a solution with a hydronium ion concentration of 1 X 10^-14 (one times 10 to the negative fourteen) moles per liter is _____. | 14 (remember, pH is equal to the negative log of the hydronium ion concentration) |
| The pH of a solution with a hydronium ion concentration of 1 mole per liter is ____. | Zero (1 mole per liter can also be expressed as 1 X 10^0, because 10 to the zero power = 1. When you express the hydonium ion concentration in scientific notation, as long as the it is 1 X 10^-n, the pH will be n) |
| Another name for intermolecular forces is _________. | Van der Waals Forces |
| Another name for a Van der Waals force is a(n) ______. | intermolecular forces |
| Intermolecular forces are weak forces ______ molecules. | between |
| What are the three types of Van der Waals forces? | 1) Dipole-Dipole (like those between polar water molecules) 2) Dipole-Induced Dipole 3) Induced Dipole - Induced Dipole (a.k.a. London Dispersion Forces) |
| The strongest type of dipole - dipole intermolecular force is called a(n) _______. | hydrogen bond |
