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Definition
| The study of composition, structure, and properites of matter. Includes the processes that matter undergoes and the energy changes that accompany these processes. |
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Definition
A change in which one or more substances are converted into different substances.
evidence of a chemical change - Burning |
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| a change in the substance that does not involve a change in the identity of the substance |
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| Is a phase change a physical change? |
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Definition
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| Homogenous Mixture/ 3 examples |
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Definition
| Homogenous mixtures are solutions, and are uniform in composition/same throughout. Examples would be sugar water, salt water, air, alloy, or milk. |
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| Heterogeneous Mixture / 3 examples |
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Definition
| Heterogenous mixture is not uniform throughout, examples would be pizza, polluted water, or cement. |
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Definition
| Conductive, thermal, electrical, malleable, ductile, luster, hardness, and most are solid. |
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Definition
| Semi conductors, brittle, break apart, soft, located in between metals and non metals. |
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| Non conductors, brittle if solid, many are gases, stable family 18, noble gas, and a low boiling point. |
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| Elements on the periodic table are listed by _____________ |
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Definition
| A testable statement that serves as a basic for making predictions and for carrying out further experiments. |
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Definition
| A broad generalization that explains a body of facts |
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| Independent/Dependent Variables |
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Definition
Independent are variables that stand alone and is not changed by any other variables.
Dependent are variables that depend on other factors. |
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| What is the purpose of the scientific method? |
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Definition
Its a logical approach to solving problems by observing and collecting data, formulating hypothesis, and formulating theories that are supported by data.
O H E M P |
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| What is a qualitative statement and a quantitative statement. |
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Definition
| Qualitative are not numerical statements and Quantitative are numerical statements. |
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| Difference between mass and weight |
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Definition
| Mass does not depend on gravity it is the measure of amount of matter when weight does depend on gravity, it is the measure of the gravitational pull on matter. |
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Term
What are the SI units for the following -
Mass -
Volume -
Density -
Length - |
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Definition
Mass -Kilogram (Kg)
Volume - Cubic meter (Cm3, Lm3)
Density - Grams per Cm3 (g/cm3)
Length - Meters (m) |
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| List the 'King Henry' prefixes |
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Definition
| Kilo, Hecto, Deca, M (Units), Deci, Centi, Milli |
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Term
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Definition
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Term
| What are the 5 statements in Daltons atomic theory? |
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Definition
1. All matter is composed of extremely small particles called atoms.
2. Atoms of a given element are identical in size, mass, and other properties; Atoms of different elements differ in size, mass, and other properties.
3. Atoms can be subdivided, created, or destroyed.
4. Atoms of different elements combine in simple who number ratios to chemical compounds
5. In chemical reactions, atoms are combined, seperated, or rearranged. |
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| What is the law of definite proportions? |
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Definition
| Every pure substance always contains the same elements combined in the same proportions by mass regardless of the size. |
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| Define the law of multiple proportions. |
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Definition
| If two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers. |
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Term
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Definition
| The smallest particle of an element that retains the chemical properties of that element. |
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Term
| Who first found the electron? What instruments were used in the experiment? |
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Definition
| JJ Thomson found the electron by using the cathode ray tube and a magnet and a paddle wheel to show the beam had mass. |
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Term
| Who first found the nucleus and what was the experiment called? |
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Definition
| Rutherford found the nucleus and called the experiment Gold foil experiment. |
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Term
| What did Rutherford conclude about the atom? |
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Definition
| He concluded that the atom is mostly empty space with a small dense center, he also found that it has a positively charged center. |
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Term
| Who developed the first periodic table? |
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Definition
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| Who made the modern periodic table? |
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Definition
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| How did the first two periodic tables differ? |
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Definition
| The first one was arranged by mass and the second was arranged by atomic mass. |
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| What is the periodic law? |
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Definition
| A principle that chemical properties of the element are periodic functions of their atomic numbers. |
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Definition
| Atoms of the same element that have different masses. |
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Term
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Definition
| A general term for a specific isotope of an element. |
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Term
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Definition
| The chemist dozen, instead of 12 units of something it is 6.02x10 23 units of something |
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| What is the average atomic mass? |
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Definition
| It is the weighted average of the atomic masses of the naturally occuring isotopes of an element. |
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Term
| How do you write hyphenated and nuclear symbolization of isotopes? |
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Definition
Hyphenated notation is when the mass is written with a hyphen after the name of the element.
Nuclear symbolization is when the superscript indicates the mass number of protons and neutrons and the subscript indicates the atomic number (#of protons) |
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| What is the electomagnetic radiation? |
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Definition
| A form of energy that exhibits wavelike behavior as it travels through space. (travels in waves) |
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| What is the relationship between wavelength and frequency? |
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Definition
| The longer the wavelength the lower the frequency. |
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| A long wavelength is high or low energy? |
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Definition
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Term
| Heisenberg Uncertainty Principle |
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Definition
| It is impossible to determine simultaneously both the position and velocity of an electron or any other particle. |
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Term
| What is an excited electron? |
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Definition
| A state in which an atom has a higher potential energy than it has in its ground state. |
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Term
| What is the quantum theory? |
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Definition
| Is describes mathematically the wave properties of electrons and other very small particles. |
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Term
| Who came up with the mathematical equation that describes as waves? |
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Definition
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Term
| What are the four quantum numbers and what do they each describe. |
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Definition
1. Principle quatum number- symbolized by n and indicates the main energy level occupied by the electron.
2. Angular Momentum Quantum Number- symbolized by l, indicated the shape of the orbital.
3. Magnetic Quantum Number- symbolized by m, indicated the orientation of an orbital around the nucleus.
4. Spin Quantum Number- has only two possible values (+1/2, -1/2) which indicate the two fundamental spin states of an electron in an orbital. |
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Term
| What are the four sublevels used in the electron configurations? |
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Definition
| s shape, p shape, d shape, and f shape. |
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| How many orbitals are in each sublevel? |
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Definition
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Term
| What is Pauli's exclusion principle? |
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Definition
| No electron can have the exact same set of 4 quatum numbers. The last designation is the spin number. |
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Term
| What is the Aufbau principle? |
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Definition
| An electron occupies the lowest energy level that can recieve it. |
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| What are the main group elements? |
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Definition
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Term
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Definition
| An atom, radical, or molecule that has gained or lost one or more electrons and has a negative or positive charge. |
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Term
| What is the noble gas configuration? Why are the noble gases stable? |
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Definition
| The noble gas configuration is a confined way of the electron configuration. They are stable because they have all their electrons. |
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| What is the most electronegative atom? |
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Definition
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