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PS Koble Exam 1
Phsical Science Koble academy exam 1
| Question | Answer |
|---|---|
| Scientific Theory | A well-tested explanation for a set of observations or experimental results. |
| Scientific law | A statement that summarizes a pattern found in nature |
| Scientific theory VS. Scientific law | A scientific law describes an observed pattern in nature without attempting to explain it. The explanation of such a pattern is provided by a scientific theory. |
| Significant Figures | All the digits that are known in a measurement, plus the last digit that is estimated. 5.25 has three significant figures. 5 has one significant figure. The fewer the significant the less precise the measurement is. |
| Precise calculation | The precision of a calculated answer is limited by the least precise measurement used in the calculation. |
| Accuracy | The closeness of a measurement to the actual value of what is being measured. |
| Compound | A substance that is made from two or more simpler substances and can be broken down into those simpler substances. |
| Pure substance | Matter that always has exactly the same composition. |
| Type of Mixtures | Heterogeneous: the parts of the mixture are noticeably different from one another. Homogeneous: the substances are so evenly distributed that it is difficult to distinguish one substance in the mixture from another. |
| Colloid | A thing that contains some particles that are intermediate in size between the small particles in a solution and the larger particles in a suspension. |
| Chemical Properties | This can be observed only when the substances in a sample of matter are changing into different substances. |
| Chemical property | Any ability to produce a change in the composition of matter. |
| Three common evidence for chemical change | A change in color, the production of gas, and the formation of a precipitate. |
| Chemical change | Occurs when a substance reacts and forms one or more new substances. (like a cake baking, leaves on a tree changing color, and food digesting in your stomach.) |
| Chemical change VS. Physical Change | When matter undergoes a chemical change, the composition of the matter changes. When matter undergoes a physical change, the composition of the matter remains the same. |
| Kinetic Theory of matter | All particles of matter are in constant motion. |
| Collisions between particles of a gas and the walls of the container cause: | The pressure in a closed container of gas. Factors that affect the pressure of an enclosed gas are its temperature, its volume, and the number of its particles. |
| Temperature: | raising the temperature of a gas will increase its pressure if the volume of the gas and the number of particles are constant. |
| Number of Particles: | Increasing the number of particles will increase the pressure of a gas if the temperature and the volume are constant. |
| The arrangement of molecules in water, at different phases. | The arrangement of molecules in water become less orderly as water melts and more orderly as water freezes. |
| Thompson's theory of matter | Thompson's experiments provided the first evidence that atoms are made of even smaller particles. Thompson said that the negative charges were evenly scattered throughout an atom filled with positively charged mass of matter. |
| Rutherford model. | According to this model, all an atom's positive charge is concentrated in its nucleus. |
| Isotopes | Atoms of the same element that have different numbers of neutrons and different mass numbers. |
| Isotopes mass number. | These of an element have the same atomic number but different mass numbers because they have different numbers of neutrons. (every atom of oxygen has 8 protons, some oxygen atoms have 8 neutrons and a mass number of 16) |
| Viscosity | The tendency of a liquid to keep from flowing -its resistance to flowing- |
| Conductivity | A material's ability to allow heat flow. |
| Malleability | The ability of a solid to be hammered without shattering. |
| Measure of hardness: One way to compare the hardness of two materials is | To see which of the materials can scratch the other. |
| Melting point and boiling point. | The temperature at which a substance changes from a solid to a liquid is its melting point. The temperature at which a substance boils is its boiling point. |
| Density | it is the ratio of the mass of a substance to its volume and it can also be used to test the purity of a substance. g/cm^3 |
| Flammability | A material's ability to burn in the presence of oxygen. |
| Reactivity | The property that describes how readily a substance combines chemically with other substances. |
| Phase change | The reversible physical change that occurs when a substance changes from one state of matter to another. |
| Fusion | another term for melting. |
| Vapor pressure | As the water evaporates, water vapor collects above the liquid. The pressure caused by the collisions of this vapor and the walls of the container is called vapor pressure. vapor pressure of water increases as the temperature increases. |
| Ground state | When all the electrons in an atom have the lowest possible energies. |
| Factors that affect the pressure of an enclosed gas are: | Its temperature, its volume, and the number of its particles. |
| Volume | Reducing the volume of a gas increases its pressure if the temperature of the gas and the number of particles are constant. |
| The periodic tables elements are arranged: | In order of increasing mass so that elements with similar properties are in the same column. |
| Periodic Table: | an arrangement of elements in columns, based on a set of properties that repeat row to row. |
| Examples of alkali metals: | Lithium, Sodium, Potassium, Rubidium, Cesium, and Francium. |
| The reactivity of alkali metals: | Increase from the top to the bottom. |
| Alkaline earth metals have: | Two valence electrons. |
| Examples of alkaline earth metals: | Beryllium, Magnesium, Calcium, Strontium, barium, and Radium. |
| Valence electron: | An electron that is in the highest occupied energy level of an atom. |
| Each Halogen has: | Seven valence electrons. |
| Nobel Gases | Colorless and Odorless and extremely unreactive. |
| examples of Nobel Gases: | Helium, Neon, Argon, Krypton, Xenon, and Radon. |
| Nobel Gases have: | Helium has two valence electrons. Each of the other has 8 valence electrons. |
| Scientific notation is: | A way of expressing a value as the product of a number between 1 and 10 and a power of 10. |
| Scientific notation makes: | Very large or very small numbers easier to work with. |
| How to use Scientific Notation for numbers less than 1: | The exponent is negative. The negative exponents tells you how many decimals places there are to the left of a number. |
| How to use scientific Notation when multiplying numbers: | Multiply the numbers that appear before the multiplication signs and add the exponents. |
| How to use scientific Notation when dividing numbers: | divide the numbers that appear before the exponential terms and subtract the exponents. |
| To convert degrees F (Fahrenheit) to Degrees C (Celsius)you: | F= 9/5 (C) + 32.0 |
| To convert degrees C (Celsius) to degrees F (Fahrenheit) | C= 5/9 (F-32.0) |
| To convert Celsius to Kelvin | K= C+273 |
| Most common ways to separate mixtures based on physical properties are by: | Solutions, Suspensions, and Colloids. |
| The three major states of matter are: | solids, Liquids, and Gases. |
| Kinetic theory related to Gas: | Each atom moves in a straight line until it collides with the other atom or wall of the container. During a collision, one atom may lose kinetic energy and slow down while the other gains kinetic energy and speeds up. total kinetic energy remains the same |
| Motion in Gases: | There are forces of attraction among the particles in all matter. |
| Kinetic theory of Gases: | The constant motion of particles in a gas allows a gas to fill a container of any shape or size. |
| Kinetic theory related to liquid: | It takes the shape of its container because particles in it can flow to new locations. The volume is constant because forces of attraction keep the particles close together. |
| Explaining the behavior of liquid: | The particles in liquid are more closely packed than the particles in a gas.therefore, attractions between the particles do affect the movement of the particles.there is a kind of tug of war between the constant motion of particles and their attractions. |
| density,mass,and volume relationship. | Density: the ratio of an object's mass to its volume. Density= mass/volume |
| temperature does not change during a phase change because: | temperature will remain at melting point until object is melted. Temperature will remain at the object's freezing point until all the liquid freezes. The melting point and freezing point are the same. |
| Bohr's model of the Atom: | The electrons move in spherical orbits at fixed distances from the nucleus. |
| Since scientist must deal with probability when trying to predict the locations and motions of electrons in an atom. Bohr's model was improved as scientists made further discoveries by the electron cloud: | visual model of most likely locations for electrons in atom.cloud is denser at those locations where probability of finding an electron is high.Scientists use the electron cloud model to describe the possible locations of electrons around nucleus. |
| Bohr's was wrong in and right in: | Assuming that the electrons moved like planets in a solar system. assigning energy levels to electrons. Today scientist know that electrons move in a less predictable way. |
| Properties of elements are affected in their arrangement on the periodic table: | Across a period from left to right, the elements become less metallic and nonmetallic in their properties. |
| Atomic mass: | A value that depends on the distribution of an element's isotopes in nature and the masses of those isotopes. |
| Atomic number: | an element equals the number of protons in an atom of that element. |
| Atoms of different elements have: | different numbers of protons. atomic number 16 because it has 16 protons. |
| Mass number of an atom is: | The sum of the protons and neutrons in the nucleus of that atom. |
| Number of Neutrons: | Number of neutrons= Mass number- atomic number |
| Identify parts of a element on the periodic table: | atomic number: top; element symbol: below atomic number; element name below element symbol; atomic mass is below the element name. |
| Group | each column on the periodic table. the elements in it have similar properties. An element's electron configuration determines its chemical properties |
Created by:
kuro98
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