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1 Matter
| Question | Answer |
|---|---|
| It is anything that occupies space and has a mass. | Matter |
| It is the physical material of the universe | Matter |
| It is the study of matter (composition, structure and properties), the changes it undergoes, and the energy involved in these changes | Chemistry |
| A state of matter; molecules that are arranged in regular repeating patterns and are held firmly in place but can vibrate within a limited area | Solid |
| A state of matter; its molecules flow easily around one another. Attractive forces between them keep them from flying apart. | Liquid |
| A state of matter; its molecules fly in all directions at great speeds. They are so far apart that attractive forces are insignificant | Gas |
| A state of matter; it is a mixture of the electrons and nuclei that have been lost by atoms at high temperature | Plasma |
| A state of matter; it is when Bose particles significantly slow down to form a condensate at extremely low temperatures | Bose-Einstein condesate |
| True or false. Kinetic energy is nearly negligible near absolute zero temperature | True |
| Classification of matter in which it gas a fixed composition and distinct qualities | Pure substance |
| Can you physically separate pure substances? | No |
| A type of pure substance that cannot be separated chemically into simpler substances | Element |
| Substance that could still be chemically separated which is composed of two or more elements in fixed properties. | Compound |
| A classification of matter which consists of two or more pure substances but still retain their individual properties | Mixture |
| Can you physically separate mixtures? | Yes |
| Mixture having uniform composition and properties throughout (aka solutions) | Homogeneous mixture |
| Mixtures that don’t have uniform composition and properties throughout | Heterogeneous mixtures |
| How many phases should a homogeneous mixture have? How about heterogeneous mixtures? | One; and more than one |
| Building blocks of matter that is unique for every element | Atoms |
| A combo of atoms with different composition and structure | Molecules |
| A property of matter that describes how a substance may react or change to form another substance | Chemical properties |
| Give some examples of chemical properties | Heat of combustion, toxicity, chemical stability, oxidation states, flammability, coordination number, reactivity, possible chemical bonds, enthalpy of formation, etc. |
| A property of matter that are observed to not have any chemical alteration to the substance of interest | Physical property |
| Type of physical property that observes things like the physical state of matter, its color, odor, crystal shape, malleability, etc. | Qualitative property |
| Type of physical property of matter that can be numerically observed and measured—e.g., melting and boiling points, density, solubility, electrical conductivity, etc | Quantitative property |
| A physical property type of matter that does not depend on the amount of sample. | Intensive property |
| It is a type of matter’s physical property that is usually dependent on the amount of sample of the substance. | Extensive property |
| What do you call the change of matter where a substance transforms into a chemically different substance? | Chemical change |
| A change of matter in which a substances changes its composition or identity | Chemical change |
| When a substance changes it physical appearance but not its composition nor identity, what change of matter occurred? | Physical change |
| It is the capacity or ability of matter to do work; may also refer to the elicit change in matter | Energy |
| The original French for SI units | Systéme Internationale d’Unités |
| In English, SI units is also called | International System of Units (or the metric system) |
| What happened on May 20, 2019 when the change of definition of some SI base units took effect? | 26th General Conference on Weights and Measures |
| Name the seven (7) SI defining constants | Transition frequency of C_s, speed of light in vacuum, Planck’s constant, elementary charge, Boltzmann’s constant, Avogadro’s constant, Luminous efficacy |
| [Hard] Identify the symbol, unit and numerical value of the transition frequency of C_s | Delta v_cs 9,192,631,770 Hz |
| [Hard] Identify the symbol, unit and numerical value of the speed of light in vacuum | c 299,792,458 m•s^-1 |
| [Hard] Identify the symbol, unit and numerical value of the Planck’s constant | h 6.62607015 x 10^-34 J•s |
| [Hard] Identify the symbol, unit and numerical value of the elementary charge | e 1.602176634 x 10^-19 C |
| [Hard] Identify the symbol, unit and numerical value of the Boltzmann’s constant | k 1.380649 x 10-23 J•K^-1 |
| [Hard] Identify the symbol, unit and numerical value of the Avogadro’s constant | N_A 6.02214076 x 10^23 mol^-1 |
| [Hard] Identify the symbol, unit and numerical value of the luminous efficacy | K_cd 683 lm•W^-1 |
| What are the names of the seven SI base units and what physical quantity are they for respectively? | Mass (kilogram kg), length (meter m), time (second s), temperature (Kelvin K), amount of substance ( mole mol), electric current (Ampere A), luminous intensity (candela cd) |
| It describes the quantity of matter an object has (a measurement of matter) | Mass |
| It is a measure of matter which describes the force of gravity acting on an object’s mass | Weight |
| It is the quantity that indicates the amount of matter per unit volume of a sample | Density |
| It is a measure of matter which refers to the percent of a component in relation to the total mass of a compound | Percent composition |
| It is the measure of the hotness or coldness of an object which also determines the direction of heat flow | Temperature |
| True or false. A hotter object is expected to have a higher temperature | True |
| It refers to the energy in transit from a region of higher temperature to a region of lower temperature | Heat |
| How do you convert °C to K? | K = °C + 273.15 |
| How do you convert °C to °F? | °F = (9/5)(°C) + 32 |
| It is used to convert from one unit to another without changing the actual property measured by multiplying with unit factors | Dimensional analysis |
| True or false. In Dalton’s atomic theory, each element is not composed of extremely small particles called atoms. | False. Look out for the word ‘not.’ |
| True or false. In Dalton’s atomic theory, all atoms of a given element are identical, and the atoms of an element may be the same to other elements | False. All atoms of a given element are identical. But the atoms of one element ARE DIFFERENT from the atoms of ALL OTHER elements |
| True or false. Dalton’s atomic theory proposed that in chemical reactions, atoms of one element cannot change into atoms of another element—atoms are either created or destroyed in these reactions. | False. Atoms are NEITHER created NOR destroyed during chemical reactions. |
| True or false. According to Dalton’s atomic theory, you can form mixtures when atoms of more than one element are combined; and a given mixture has always the same relative number and kinds of atom. | False. It is not mixture, it is COMPOUND. |
| Who proposed the Law of Conservation of Mass? | Antoine Lavoisier |
| The law that states matter is neither created nore destroyed during chemical or physical reactions | Law of Conservation of Mass |
| Who proposed the Law of Definite Composition? | Joseph Louis Proust |
| The law that says, “a compound always contains elements in a certain proportion by mass (constant composition).” | Law of Definite Composition |
| Who proposed the Law of Multiple Proportions ? | John Dalton |
| In this law, it is proposed that regardless of its source, a pure compound will always have the same composition of elements and the same properties—they will always have same ratio | Law of Multiple Proportions |
| He discovered the electrons in 1897. | J. J. Thompson |
| These are beams which pass from the negative electrode of the ray tube to the positive electrode. | Cathode rays |
| The negative terminal of the cathode ray tube | Cathode. |
| This refers to the positive terminal of the cathode ray tube. | Anode |
| [Hard] What is J. J. Thompson’s calculation of the charge-to-mass ratio of electrons. | –1.76 x 10^8 C•g^-1 |
| What are the three (3) types of radiation that Ernest Rutherford revealed? | Alpha, beta, gamma |
| J. J. Thompson’s experiment that lead him to the discovery of electrons | Cathode-ray tube experiment |
| Who discovered the mass of electrons in 1909? | Robert Millikan |
| Robert Millikan found the electrons’ mass by using Thompson’s ratio. What was the calculated mass? | 9.10 x 10-28 g |
| The experiment that lead Robert Millikan to discover the electron’s mass. | Oil-drop experiment |
| In 1896, he found out that uranium emits high energy radiation. | Henri Becquerel |
| They conducted series of experiments which made them discover that uranium atoms causes radiation. Hint: they’re a couple and the wife was the first woman to win the Noble Prize. | Marie Curie and Pierre Curie |
| An atomic model proposed by J. J. Thompson (early 1900s) in which negatively charged electrons are supposed to be dispersed in a positively charged sphere (or cloud) of matter. | Plum-pudding model. |
| He discovered the nucleus and proton. | Ernest Rutherford |
| The experiment used by Ernest Rutherford to discover the protons and nucleus of atoms. | Gold-foil experiment |
| What is the other term for the gold-foil experiment? | alpha-scattering experiment |
| In 1932, he discovered the neutrons of atoms | James Chadwich |
| These are small neutral particles in the atomic nucleus whose mass is the same with protons. | Neutrons |
| It refers to the number of protons in an element. It is also mainly holds the overall characteristic of the element | Atomic number |
| Symbol for the atomic number | Z |
| Refers to the sum of protons and neutrons in the nucleus. Contains the information of the isotopic nature of the elements | Mass number |
| Symbol for mass number | A |
| These are charged particles when an atom loses or gains electrons. | Ions |
| These are the negatively charged ions when an atom gains electrons | Anions |
| When atoms lose electrons, they give the positively charged ions called | Cations |
| These are atoms of the same element but having different numbers of electrons, hence different masses. | Isotopes |
| Can you drop the atomic number Z when writing isotopes? | Yes |
| It is equal to the mass of 1/12 of carbon-12 | Atomic mass unit |
| [Hard] How many grams is one (1) amu? | 1 amu = 1.66054 x 10^-24 |
| [Hard] How much amu does a gram have? | 1 g = 6.02214 x 10^34 |
| It refers to the weighted sum (average) of the isotopic masses of an atom times their relative abundance in nature. | Average atomic mass |
| The other term for the average atomic mass | Atomic weight |
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