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Chem Midterm
Vocabulary for Chemistry
| Term | Definition |
|---|---|
| The Scientific Method | 1. Ask a Question 2. Do background research 3. Construct hypothesis 4. Test with experiment 5. Report results |
| Qualitative Data | A type of informal data described in terms of quality or categorization such as warmth and flavor |
| Quantitative Data | A type of data described in terms of quantity where numerical values are used. |
| Chemistry | The study of Matter |
| Hypothesis | an educated guess that explains observations |
| The manipulated variable | the variable that is deliberately changed in an experiment |
| Volume | The amount of space an object occupies |
| Mass | The amount of matter in an object |
| Unit of messure for Mass | Gram |
| Unit of messure for Temperature | Celsius |
| Unit of messure for Volume | Liter |
| Unit of messure for Length | Meter |
| How many cm^3 = 1 mL | 1 cm^3= 1 mL |
| King Henry Dies Unexpectedly Drinking Chocolate Milk (m) | Kilo, Hexa, Deca, Unit, Deci, Centi, Milli, micro |
| 1,000,000 ug(micrograms)/ gram | |
| Physical Change | Any change not involving a change in the substances chemical make-up |
| Chemical Change | A change involving the atomic and molecular structure of a substance |
| Physical Property | Property os a compound that can change without involving a change in chemical composition |
| Chemical Property | Property that changes the chemical make-up of a substance |
| Element | Substance composed of atoms having an identical number of protons in each nucleus. Cannot be reduced to simpler substances by normal chemical means |
| Compound | Substance containing two or more elements and cannot be seperated by physical means |
| Pure subsance | A sample of matter, either an element or a compound, with definite physical properties and a definite composition |
| Mixture | Composed of two or more substances that are not chemically combined and can be seperated |
| Heterogeneous Mixture | A mixture that is not uniform in structure and composition |
| Homogeneous Mixture | A mixture that is uniform in structure and composition. Often called a Solution |
| Alloy | A homogeneous mixture of two metals |
| Ways of seperating parts of a mixture | Magnetism, evaporation, filtration, distillation, and centrifuge |
| Plasma | Superheated gas |
| Melting Point | Solid to liquid. Same as feezing point |
| Freezing point | Liquid to solid. Same as Melting Point |
| Condensation point | Gas to Liquid |
| Sublimation point | Solid to Gas |
| Law of conservation of Mass | Mass can neither be created nor destroyed in a reaction |
| Density Formula | D=M/V. Where D=density, M=Mass, and V=Volume |
| Density of water | 1g/cm^3 |
| Atomic Number | The number of protons in an element. Increases across and increases down the periodic table. |
| Atomic Mass | The avarage of the masses of all the element's isotopes. . Increases across and increases down the periodic table. |
| The number of protons in a nucleus equals... | the number of electrons |
| Isotope | An element that has a different number of nuetrons than normal |
| Mass number | The total number of protons and neutrons in an atom |
| Nucleon | The particles in the nucleus of an atom |
| A proton has a _______charge | positive |
| A nuetron has_______ | no charge |
| An electron has a__________charge | negative |
| Dalton | Developed the first modern atomic theory |
| Bohr | Postulated that electrons were in fixed paths in fixed energy levels and developed the model of an atom |
| Planck | Postulated the term "quanta" to explain light |
| The speed of light | 3 x 10^8 |
| Spectroscope | an instrument that allows you to see bands of color in a reaction |
| Orbital | The region of space where an electron is liekly to be found |
| Dalton's Atomic Theory part 1 | All matter is composed of atoms. All atoms of an element are identical, atoms of different elements are different. |
| Dalton's Atomic Theory part 2 | Chemical reactions involve the combination of atoms, not the destruction. When elements react to form compounds, they react in defined, whole number ratios. |
| Wavelength formula | λ (wavelength)= v(volume)/f(frequency) |
| Ground level | Electrons in the lowest energy levels and closest to the nucleus |
| 2 Modern Views of light | 1. Light moves as waves 2. Light moves as a stream of particles |
| Mendeleev | Discovered the first periodic table and arranged it by increasing atomic mass |
| Moseley | Arranged the periodic table by increasing atomic number |
| Mendeleev and Moseley | Created th modern periodic law which states that the properties of elements repeat in a pattern when elements are arranged by increasing atomic number |
| Elements in a column | have the same number of valence electrons |
| Nobel gases | Gases whose outer-most energy levels are full and do not bond with other elements |
| Metalloid | What is the term for elements with both metal and non-metal characteristics |
| Atomic radius | The distance from the nucleus to the outer shell. Calculated by finding the half the distance between nulei of two like atoms. Decreases across and increases down the periodic table. |
| Ionization Energy | the energy required to remove an electron from a neutral atom. Increases across and decreases down the periodic table. |
| Ion | A charged atom |
| Ionic | The type of bonding that involves a transfer of electrons and produces substances that are hard, or difficult to crush. |
| Covalent | the type of bounding that results in volitle liquids |
| Metallic | bonding produces substances that have luster. |
| Cation | When an atom loses electrons |
| Anion | When an atom gains electrons |
| Avogadro’s number | 6.02x10^23 |
| Molar Mass | The mass of one mole of any pure substance |
| The empirical formula | represents the simplest whole number ratio of atoms |
| The molecular Formula | represents the actual number of each atom in the compound. |
| hydrates | compounds that crystallize from a water solution with water molecules clinging to the crystal particles. |
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