Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
PhySci EOC List 1
| Question | Answer |
|---|---|
| The larger an object's mass, the (larger or smaller) the inertia? | Larger |
| What is the tendency of matter to resist change in motion? | inertia |
| What happens to a solid object whose density is less than water and it is placed in the water? | it sinks to the bottom |
| What is weight? | the gravitational force on an object |
| After pouring 3 liquids into a beaker, the green one sinks to the bottom. What would that tell you? | The green liquid is the densest |
| What does the volume tell us? | the amount of space an object occupies |
| What does mass tell us? | it measures the amount of mass in an object |
| The explosion of fireworks is an example of what kind of change? | chemical change |
| Changes of state (solid to liquid to gas) is an example of what kind of change? | physical change |
| Something that is malleable is what? | is able to be made into thin sheets |
| What is the relationship of volume and mass? | density |
| What is electrical conductivity? | the ability to conduct an electric currect |
| A change in form that does not change a substances identity is called this.. | physical change |
| When a substance has changed into a new substance we know that this kind of change has taken place... | chemical change |
| Reactivity is a part of a(physical or chemical) change | chemical |
| What is solubility? | the ability of a substance to dissolve |
| What is a physical property? | a property that can be observed or measured such as color, state or hardness |
| What are some examples of a chemical change? | rusted metal, sour milk, digested food |
| What is reactivity? | the ability of a substance to combine and form other substances |
| What is flammability? | the ability of a substance to burn |
| Why does ice float in liquid water? | The ice's density is lower than the water |
| How do you find the density of an object? | Mass/Volume |
| physical change | a change that does not result in a new substance |
| chemical change | a change or reaction that creates a new substacne |
| solid | always viberating close together |
| liquid | moves somewhat fast not very close |
| gas | fast and far apart |
| plasma | super hot and only is stars and lightning |
| vaporization | liquid to gas |
| condesation | gas to liquid |
| freezing | liquid to solid |
| melting | solid to liquid |
| atom | smallest particale that can be called an element cant be seperated any further has protons neutrons and electrons |
| element | pure substance cant be broken- no two are the same |
| nucleus location | center of an atom |
| proton | positive in the nucules the atomic number |
| neutron | neutral charge in the nuclues the atomic mass rounded minus the atomic number |
| electron | negetive in the cloud around the nuclues atomic number |
| non metals | not mallible or conductive low density and low melting point |
| metals | conduct heat and electricity are malliable |
| groups on per. table | alkiai; alkiali earth metals; transiton metals; inner transtion metals; halogens; noble gases |
| atomic number | number or protons and electrons |
| atomic mass | protons + neutrons |
| atomic symbol | idenification |
| isotope | the possible different versions of an element |
| ionic bond | opposite charged atoms stick together |
| covalent bond | bond when 2 atoms share a valence electron |
| Mass Number | Protons + Neutrons |
| Atomic Number | Protons |
| - 1 charge | Electron |
| Mass Number - Atomic Number | Neutrons |
| Particles with significant mass | Protons and Neutrons |
| Determines what element an atom is | Protons |
| Exist in a "cloud" | Electrons |
| Are found in the nucleus | Protons and Neutrons |
| Changing these will only change the mass of the atom | Neutrons |
| Changing these will change the charge of an atom but not the mass | Electrons |
| Changing these will change the type of atom | Protons |
| Particles on the highest energy level | valence electrons |
| Highest number of electrons in a valence shell | 8 |
| These match the number of protons in a neutral atom | electrons |
| An atom with a charge (not neutral) | ion |
| These are gained or lost to form an ion | electrons |
| An atom that has gained electrons | Anion |
| An atom that has lost electrons | Cation |
| Compare these particles to discover the charge of an atom | Protons and Electrons |
| Types of Pure substances | Elements and Compounds |
| Elements in Group 1 | Alkali Metals |
| Elements in Group 2 | Alkaline Earth Metals |
| Elements in Group 3-12 | Transition Metals |
| Elements in Group 17 | Halogens |
| Elements in Group 18 | Noble (or Inert) Gases |
| Elements on the left side of the Periodic Table (Most of the elements) | Metals |
| Elements on the right side of the Periodic Table | Nonmetals |
| Columns on the periodic table are called | Groups |
| Rows on the periodic table are called | Periods |
| You look at this on the periodic table to know how many energy levels an atom has | Periods |
| You can look at this on the periodic table to quickly know how many valence electrons an atom has | Groups |
| This is what determines the order of elements on the periodic table | Atomic Number |
| 2 or more elements chemically bonded together | Compound |
| 2 or elements physically put together | Mixture |
| Water is classified as a ... | Compound |
| Air is classified as... | Mixture |
| Homogeneous mixtures are usually | Solutions |
| Elements are represented by... | Symbol |
| Compounds are represented by... | Formula |
| Elements here have 3 valence electrons | Group 13 |
| Elements here have a full valence | Group 18 |
| Elements here have 1 valence electron | Group 1 |
| Elements here want to gain 1 electron | Group 17 |
| Elements here want to lose 1 electron | Group 1 |
| Elements here want to lose 3 electrons | Group 13 |
| Brittle, often gas at room temperature, non-conductive | Nonmetals |
| Shiny, malleable, conductive | Metals |
| How is the periodic table arranged? | Atomic number (protons). |
| What are the rows called? | A period. |
| How are periods determined? | By the amount of energy levels. |
| What are columns called? | Groups or families. |
| How are groups and families determined? | By the amount of valence electrons. |
| What's the oxidation number of Alkali Metals Family? | 1 |
| What's the oxidation number of Alkaline Earth Metals Family? | 2 |
| What's the oxidation number for the Boron Family? | 3 |
| What's the oxidation number for the nitrogen family? | -3 |
| What's the oxidation number for the Oxygen Family? | -2 |
| What's the oxidation number for the Halogens family? | -1 |
| What's the oxidation number of the Noble Gases Family? | 0 |
| What are valence electrons? | They are on the very last/outside energy ring of an atom. |
| What is a stable atom? | When all of its energy levels are filled. |
| Where are the most reactive metals? | To the left and down the table. Alkali Metals. |
| Where are the most reactive nonmetals? | To the right and up the table. Halogens. |
| What are the most nonreactive elements? | The Noble Gases. |
| What is the zigzag line? | Metalloids. |
| What's to the left of metalloids? | Metals. |
| What's to the right of metalloids? | Nonmetals. |
| How many elements are liquids at room temperature? | Two. |
| Conservation Of Mass | "Mass Cannot Be Created Or Destroyed" |
| Compound | A Mixture With Two Or More elements |
| Molecule | Group Of Atoms Bonded Together |
| Covalent Compound | Between 2 nonmetals |
| Ionic Compound | Between A Metal And Nonmetal |
| Lewis Dot Structure | way to see how compounds from using their valence electrons |
| Substance | Something that can't be changed, pure. |
| Solution | Another word for heterogenous mixture |
| precipitate | A solid formed from crystallization. |
| solute | Substance that is dissolved or seemed to disappear |
| Solvent | Substance that is dissolved from the solute |
| Heterogeneous | A mixture that is not evenly mixed |
| Homogeneous mixture | A mixture that is evenly mixed |
| physical change | when the appearance changes, not the substance |
| Vaporization | When a liquid turns into a gas |
| Condensation | gas changes to liquid |
| sublimation | solid to gas |
| deposition | gas changed to solid |
| chemical change | substances change to different substances |
| compound | two or more atoms (elements) chemically bonded together by a chemical reaction. ex. NaCl |
| covalent bond | When atoms share valence electrons to feel stable. When two non-metals bond together. |
| covalent bond properties | These are weak bonds. They have low melting and boiling points. ex. H20 |
| element | Smallest form of matter. Cannot be broken down into a smaller substance. Ex. Au |
| Group 1 | Easier to bond with because it has less valence electrons to get rid of. (1 valence e-) |
| Group 14 | Hard to bond with because it needs to add or lose 4 electrons to feel stable. |
| Group 17 | Easier to bond with because it only needs one more electron to be full. (It has 7 valence e-) |
| hydrogen bond | when water molecules bond to other water molecules. |
| ionic bond | When ions of opposite charges are attracted to one another and bond. When a nonmetal and a metal bond together. |
| ionic bond properties | These are strong bonds. They have high melting and boiling points. Ex. CaCl2 |
| ions | Atoms that gain or lose electrons and will have a positive or negative charge. |
| isotopes | Atoms that gain or lose neutrons. They will have a neutral charge and their mass will change. |
| Law of Conservation of Mass | Mass cannot be created or destroyed. This means the mass before a chemical reaction has to be the same after a reaction. |
| metallic bonds | When two metal atoms bond together by loosely held together valence electrons. They conduct electricity, have luster, are malleable, and ductile. |
| metals | are on the left side of the periodic table. |
| Non-metals | are on the right side of the periodic table. |
| metalloids | Can act as a metal or a non-metal. These elements border the stair steps of the periodic table. |
| Positive Charged Ion | Happens when an atom loses electrons. |
| Negative Charged Ion | happens when an atom gains electrons. |
| Cation | A positive ion |
| Anion | A negative ion |
| Radioactivity | the spontaneous emission of radiation by an unstable atomic nucleus |
| Half-life | length of time required for half of the radioactive atoms in a sample to decay |
| What do we call an atom that has lost or gained electrons | Ion |
| An ion that has lost electrons becomes more | Positive |
| An ion that has gained electrons becomes more | Negative |
| Electrons have a positive or negative charge? | Negative |
| A positively charged ion is called a | Cation |
| A negatively charged ion is called an | Anion |
| The nucleus is made up of | Protons and neutrons |
| Protons are positively or negatively charged? | Positive |
| Atoms will lose or gain electrons in order to get a | Full outer shell |
| Elements in group 2 will always try to Lose or Gain 2 electrons? | Lose 2 electrons |
| The aluminium atom loses 3 electrons and is written as | Al+3 |
| Why do group 8 not lose or gain electrons | They already have a full outer shell |
| An isotope is an atom of an element that has a different mass number due to | A different number of neutrons in the nucleus |
| Atomic number tells us: | The number of protons in the nucleus of an atom |
| The mass number tells us: | The number of protons and neutrons in the nucleus of an atom. |
| The atomic mass of elements on the periodic table is not a whole number because: | It is the average of all the isotopes of each elements. |
| The isotope of carbon that is used in archaeology to date artifacts is called: | Carbon-14 |
| A sulfur atom with 16 protons, 16 electrons and 16 neutrons has a mass number of: | 32 |
| A sodium ion has 11 protons, 12 neutrons and has +1 charge. How many electrons does it have? | 10 |
| attractive force that holds different atoms together to make a compound | chemical bond |
| two or more elements joined together in a certain ratio | compound |
| a diagram to show how the atoms in a compound are connected; uses chemical symbols to represent the atoms | structural formula |
| results in a substance that is a strong solid with a high melting/boiling point | crystal (network structure) |
| determines whether a substance is a solid, liquid or gas at room temperature | attractions between the molecules |
| interact to form bonds between atoms | valence electrons |
| number of valence electrons to make a "full" outer shell in MOST elements | 8 |
| bonds formed when a positive ion and a negative ion are attracted to each other | ionic bond |
| form positive ions (are electron donors) | metals |
| form negative ions (are electron takers) | nonmetals |
| formed by the transfer of electrons | ionic bond |
| tells the ratio of ions in an ionic compound | formula unit |
| do not conduct electricity unless they are dissolved in water | ionic compounds |
| bonds that form between metal atoms that cause them to pack together and allow them to conduct electricity | metallic bonds |
| bonds formed between nonmetals | covalent bonds |
| bonds formed between a metal and a nonmetal | ionic bond |
| bonds formed when atoms share one or more pairs of valence electrons | covalent bonds |
| a covalent bond in which the electrons are shared equally | nonpolar covalent bond |
| a covalent bond in which the electrons are NOT shared equally, forming a sort of positive end and negative end of the molecule | polar covalent bond |
| NaCl | sodium chloride |
| K₂O | potassium oxide |
| Li₃N | lithium nitride |
| MgCl₂ | magnesium chloride |
| CaO | calcium oxide |
| Sr₃P₂ | strontium phosphide |
| BaBr₂ | barium bromide |
| Al₂S₃ | aluminum sulfide |
| Rb₂Te | rubidium telluride |
| CsCl | cesium chloride |
| In₂O₃ | indium oxide |
| Na₂Se | sodium selenide |
| KBr | potassium bromide |
| KBr | potassium phosphide |
| MgO | magnesium oxide |
| CaF₂ | calcium fluoride |
| AlI₃ | aluminum iodide |
| KCl | Potassium Chloride |
| CaBr₂ | Calcium Bromide |
| Rb₂S | Rubidium Sulfide |
| Chemical Nomenclature | the systematic naming of chemical compounds |
| Binary compound | molecule made of 2 elements |
| Prefix for 1? | Mono |
| Prefix for 2 | Di |
| Prefix for 3 | Tri |
| Prefix for 4 | Tetra |
| Prefix for 5 | Penta |
| Prefix for 6 | Hexa |
| Prefix for 7 | Hepta |
| Prefix for 8 | Octa |
| Prefix for 9 | Nona |
| Prefix for 10 | Deca |
| CO₂ | Carbon dioxide |
| N₂O5 | Dinitrogen pentaoxide |
| Ionic Bond | Electrons are transfer Loose electrons Are Cations |
| Covalent Bond | Electrons are share |
| Noble gases | element neither receives or loses electrons |
| non polar | electrons equally shared |
| polar | electrons NOT equally shared |
| Ionic bonds | dissolve easily in water form solids with high melting temperatures. conduct electricity. |
| Valence electrons | outermost electrons |
| Dinitrogen monoxide | N₂O |
| lithium iodide | LiI |
| lithium oxide | Li2O |
| lithium sulfide | Li2S |
| beryllium fluoride | BeF2 |
| beryllium sulfide | BeS |
| boron sulfide | B2S3 |
| copper (I) bromide | CuBr |
| copper (I) iodide | CuI |
| aluminum oxide | Al2O3 |
| aluminum nitride | AlN |
| aluminum phosphide | AlP |
| magnesium bromide | MgBr2 |
| magnesium oxide | MgO |
| magnesium nitride | Mg3N2 |
| potassium fluoride | KF |
| potassium oxide | K<sub>2</sub>O |
| calcium bromide | CaBr2 |
| iron (II) chloride | FeCl2 |
| What is the release of particles and energy from nuclear decay? | radioactivity |
| Why is carbon 14 radioactive? | its ratio of protons to neutrons is not stable |
| On what does the stability of an isotope’s nucleus depend? | the ratio of protons to neutrons |
| What radiation can be stopped with a sheet of paper? | alpha particles |
| What is the time it takes for the ½ of the nucleus in a radioactive sample to decay? | half-life |
| What is the process of changing one element into another through nuclear decay? | transmutations |
| What do scientists use Carbon-14 for? | to calculate the age of once living things EX: bones |
| What type of radiation penetrates thick metals and concrete? | gamma rays |
| Name the three types of radiation. | alpha, beta, gamma |
| Which type of particle occurs when high speed electrons are emitted from a nucleus? | beta particles |
| What type of radiation can be stopped with a thin sheet of metal? | beta radiation |
| What radiation is made of two protons and two neutrons? | alpha radiation |
| What happens when the strong force is not big enough to hold the nucleus together? | the nucleus decays or breaks down giving off radiation |
| What device detects radiation by producing a current and ‘clicking’? | Geiger counter |
| What did Marie Curie discover? | radioactive Radium and Polonium |
| Who discovered radioactivity and how? | Bequerel with uranium and a photographic plate |
| What radiation is electromagnetic waves with high-frequency energy? | gamma radiation |
| What causes protons and neutrons to be attracted to each other in the nucleus? | strong force |
| Why is carbon-14 radioactive? | its ratio of protons to neutrons is 6/8 |
| How does carbon dating work? | the ratio of C-12 to C-14 twlls how many half-lifes has passed |
| What is the process of splitting a nucleus into two smaller nuclei releasing a huge amounts of energy? | nuclear fission |
| What is the process of combining together 2 nuclei with low masses to make one larger one? This also releases huge amounts of energy. | nuclear fusion |
| What type of reaction is used in a nuclear power plant? | Nuclear fission reaction |
| How is nuclear fission controlled in a power plant? | control rods that absorb some of the neutrons which split atoms |
| What type of reaction takes place in the sun and stars? | Nuclear Fusion reaction |
| What is the range of atomic numbers of elements whose isotopes are all radioactive? | all elements past #83 |
| Name cons to nuclear power. | radioactive waste is produced and there is no way to store it, if something goes wrong, radioactivity is released into the environment |
| Name pros of nuclear power. | lots of energy from little fuel, no pollutants into air, no carbon dioxide released into air |
| How is radioactivity useful in medicine? | radioactive tracers used to detect problems, radiation can kill cancer cells |
Created by:
jaredlovering
Popular Physical Science sets