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Chem110 Review Test2
Review for Chem110 quiz/test for DelTech Owens
| Question | Answer |
|---|---|
| What is the basic structural unit of an element? | The atom |
| An atom is the smallest unit of an element that retains the __ of that element. | properties |
| What are the 3 primary particles of an atom? | electrons, protons, neutrons |
| A small, dense, positively charged region in the center of an atom is called the __. | nucleus |
| Protons are __ charged. | positively |
| Neutrons have a __ charge. | neutral |
| Electrons have a __ charge. | negative |
| If the electrons and protons of an atom are equal in number, the atom will have a __ charge. | neutral |
| On the periodic table, the number of protons in an atom is represented by the __ __. | atomic number |
| On the periodic table, the sum of the protons and neutrons is called the __ __. | mass number |
| On the periodic table, if there is no charge shown for an element, then its charge is __. | zero |
| To find the number of electrons for an element on the periodic table, subtract the __ __ from the __ __. | mass number from the atomic number |
| What is the mass and charge for an electron? | Charge = -1; Mass (amu)= 5.4 x 10^-28 |
| Electrons are abbreviated as __. | e |
| What is the mass and charge for a proton? | Charge = +1; Mass (amu) = 1.00 |
| Protons are abbreviated as __. | p |
| What is the mass and charge for a neutron? | Charge = 0; Mass (amu) = 1.00 |
| Neutrons are abbreviated as __. | n |
| Atoms of the same element that have different masses than the "normal" atom of that element are called __. | isotopes |
| Isotopes contain the same number of __ as a normal atom of that element. | protons |
| Isotopes have __ __ number of __. | a different number of neutrons |
| Two isotopes of hydrogen are called __ and __. | deuterium and tritium |
| Isotopes of the same element have __ chemical properties. | identical |
| Some isotopes are __. | radioactive |
| The atomic mass is really the __ __ of the masses of all the isotopes that make up the element. | weighted average |
| An average corrected by the relative amounts of each isotope present in nature is called the __ __. | weighted average (which is equal to its atomic mass) |
| The first experimentally based theory of atomic structure is called __ __ __. | Dalton's Atomic Theory |
| Which of Dalton's Atomic Theory postulates is wrong? | 2 and 3; the rest are all true. |
| What disproves the following postulate from Dalton's Atomic Theory (#2): "An atom cannot be created, divided, destroyed, or converted to any other type of atom." | radioactivity |
| What disproves the following postulate from Dalton's Atomic Theory (#3): "Atoms of a particular element have identical properties." | isotopes |
| Thomson (of Crookes and Thomson) discovered the __. | electron |
| Electrons were the first subatomic particle to be discovered. This was done using a __ __ __. | cathode ray tube |
| Experiments by __ __ and __ __ showed that the atom is composed of + and - particles. | William Crookes and Eugene Goldstein |
| When Crookes ran his experiment using a cathode ray tube, rays of lights were seen traveling between the two electrodes. The electrodes were called the __ and the __. | cathode, anode |
| The cathode in a cathode ray tube was __ (negative or positive)? | negative |
| The anode in a cathode ray tube was __ (negative or positive)? | positive |
| Later experiments by __ proved the rays were both electrical and magnetic. | J.J. Thomson |
| The ability to produce cathode rays is a characteristic of __ __. | all materials |
| It was Thomson who announced that cathode rays were really streams of negative particles of energy. These particles are __. | electrons |
| Experiments by Goldstein proved that there were particles of equal charge, but of opposite sign, to the electron. Those particles are called __. | protons |
| Neutrons have a mass almost __ to that of a proton. | identical |
| The mass of a neutron is __ __ __ __ lower than that of a proton. | less than 1% |
| Neutrons were proven to exist by __ __. | James Chadwick |
| Rutherford's __ __ experiment proved that the atom is mostly empty space. | Gold Foil |
| We use the measurement of particle __ rather than position. | energy |
| The absorption or emission of light by atoms is called __. | spectroscopy |
| Spectroscopy is used to understand the electronic __. | structure |
| Light is a form of __ __. | electromagnetic radiation |
| Electromagnetic radiation travels in __ from a source. | waves |
| The speed of light is __. | 3.0 x 10^8 m/s |
| Electromagnetic radiation goes farther if its __ are shorter. | waves |
| Light moves as a collection of __ waves. | sine |
| The distance between identical points on successive waves is called __. | wavelength |
| Each wavelength of electromagnetic radiation travels at the same __ but has its own characteristic energy. | velocity |
| Wavelengths and energy are __ related when talking about electromagnetic radiation. | inversely |
| Bohr's theory: atoms can absorb and emit energy via __ of electrons to higher energy levels. | promotion |
| Bohr's theory: when excited electrons return to lower levels of energy, this is called __. | relaxation |
| Bohr's theory: __ __ are a result of electron transitions between __ __ in the atoms. | allowed levels |
| Each electron has its own __ lines, or signature. | spectral |
| Each element has its own __ __. | electron structure |
| Spectral lines of electrons can be seen using a __. | spectroscope |
| The emission spectrum of what element lead to the modern understanding of the electronic structure of the atom? | hydrogen |
| Bohr's Atom: electrons exist in fixed energy levels surrounding the __. | nucleus |
| Bohr's Atom: promotion of electrons occurs as they absorb __. | energy |
| Bohr's Atom: energy is released as an electron travels back to __ __ once its excess energy has been used. | lower levels; this is called relaxation |
| Bohr's Atom: the amount of energy absorbed when an electron jumps from one energy level to a higher energy level is a __ quantity. | precise |
| Bohr's Atom: when an electron jumps from one energy level to a higher one, the difference between the orbits represents the __ of that jump. | energy |
| Bohr called the fixed energy levels of electrons __. | orbits |
| Bohr called the lowest possible energy level for an electron its __ __. | ground state |
| According to Bohr's theory, electrons are only found in __ levels, or obits. | allowed |
| An electron's orbit is different from an atomic __. | orbital |
| One major change between Bohr's Atomic Theory and modern Atomic Theory is that electrons do not move in __. | orbits |
| Bohr's model of the atom failed to explain their line __. | spectra |
| Electrons move rapidly within the atomic orbital giving it a high __ __. | electron density |
| The Periodic Table was invented independently by __ __ and __ __. | Dmitri Mendeleev and Lothar Meyer |
| As you list elements on the periodic table in order of atomic mass, there is a distinct regular __ in their properties. | variation |
| The physical and chemical properties of the elements are periodic functions of their atomic numbers. This is called __ __. | periodic law |
| Metalloids (as listed on the periodic table) and like metals AND __. They are intermediate substances. | nonmetals |
| On the periodic table, a horizontal row of elements is called a __. | period |
| On the periodic table, a vertical column of elements is called a __. | group |
| Elements in a particular __, or family on the periodic table, share many similarities. | group |
| If a group on the periodic table has an A in front of it, that means the column features __ __. | main-group elements |
| If a group on the periodic table has an B in front of it, that means the column features __ __. | transitional elements |
| Elements that tend to lose electrons during chemical change are called __. They form positive ions. | metals |
| A substance whose atoms tend to gain electrons during chemical change are called __. They form negative ions. | nonmetals |
| Metals are found primarily in the left __ of the periodic table. | 2/3 |
| Metals have high __ and __ conductivity. | electrical and thermal |
| Metals have high __ and __. | malleability and ductility (meaning they can be formed into thin wire) |
| Metals have a high __. | metallic luster |
| Most metals are __ at room temperature. | solid |
| Mercury, though a metal, is a __ at room temperature. | liquid |
| Nonmetals tend to gain __, forming negative ions. | electrons |
| Nonmetals can be found in the right __ of the periodic table. | 1/3 |
| Nonmetals tend to be __. | brittle |
| Nonmetals are __ solids or gases. | powdery |
| Basically, nonmetal properties are the __ of metal properties. | opposite |
| Most periodic tables give the element __, atomic __, and atomic __. | symbol, atomic number, atomic mass |
| The primary factor in understanding how atoms join together to form compounds it the __ __. | electron arrangement |
| The arrangement of electrons in atoms is atom's __ __. | electron arrangement |
| The outermost electrons in an atom, which are involved in chemical bonding, are called __ __. | valence electrons |
| Bohr's model of the hydrogen atom didn't clearly explain the electron __ __ __ __. | structure of other atoms |
| Wave properties of electrons conflict finding their specific __. | location |
| Who developed the equations that took into account the particle nature and the wave nature of electrons? | Shroedinger |
| Schroedinger's equations allow us to determine the __ of finding an electron on a specific region of space. | probability |
| Each possible energy level of an electron has one or more __ or __. | sublevels or subshells |
| Each electronic sublevel contains one or more atomic __. | orbitals (remember, orbitals differ from orbits) |
| The first 4 sublevels are designated __. | s, p, d, f |
| The higher the energy level, the __ the electron is from the atomic nucleus. | farther |
| If an electron's principle energy level is 1, then it's sublevel is __ __. | also 1 |
| The electron capacity of a principle energy level is __. | 2(n)^2 |
| When determining how many electrons can in in a sublevel, you always __ the number of the sublevel. | double |
| A set of energy-equal orbitals within a principle energy level is called a __. | sublevel |
| Electrons in the 3d subshell have __ energy than electrons in the 3p subshell. | more |
| When describing the location of an atom, you must specify both the __ __ __ and the __. | principle energy level and the subshell |
| A specific region of a sublevel containing a maximum of 2 electrons is called an __. | orbital |
| Orbitals are named by their __ and their __ __ __. | sublevel and their principle energy level |
| Each type of orbital has a characteristic __. | shape |
| The S type orbital is __ symmetrical. | spherically |
| The P type orbital has a shape like a __. | dumbbell |
| The s subshell has _ orbital, and a maximum of __ electrons. | 1 orbital, 2 electrons |
| The p subshell has __ orbitals, and a maximum of __ electrons. | 3 orbitals, 6 electrons |
| The d subshell has __ orbitals, and a max of __ electrons. | 5 orbitals, 10 electrons |
| The f subshell has __ orbitals, and a max of __ electrons. | 7 orbitals, 14 electrons |
| The arrangement of electrons in atomic orbitals is called an __ __. | electronic configuration |
| The building up principle helps determine the electron configuration. Another phrase for the "building up" principle is the __ __. | Aufbau Principle |
| Electrons fill the __-__ orbital that is available first. | lowest-energy |
| Each orbital can hold up to 2 electrons with their spins in opposite directions. This is called the __ __ __. | Pauli Exclusions Principle |
| Each orbital in a subshell is half-filled with one electron and prior to filling the orbitals with 2 electrons. This describes __ __. | Hund's Rule |
| To write an electron's configuration, you must obtain the total number of __ in the atom from the atomic number. | electrons |
| To write an electron's configuration, you must remember that electrons occupy the __ energy orbitals that are available. That means __ comes first. | lowers, 1s |
| To write an electron's configuration, you must remember that each __ __ __ contains the same number of sublevels. | principle energy level |
| To write an electron's configuration, you must remember that the s sublevel has __ orbital, the p sublevel has __ orbitals, and the d sublevel has __ orbitals. | 1,3,5 |
| To write an electron's configuration, you must remember that there can't be more than __ electrons in any orbital. | 2 |
| To write an electron's configuration, you must fill orbitals from __ to __ energy. | lowest to highest |
| To write an electron's configuration, you must remember that the max number of electrons in any principal energy level is __. | 2(n)^2 |
| Noble gases are extremely __. | stable |
| Noble gases are called __ because they don't readily bond to other elements. | inert |
| The stability of noble gases is due to a full complement of __ __ in the outermost s and p sublevels. | valence electrons |
| Elements usually react in such a way as to attain the electron configuration of the noble gas closest to them in the periodic table. This is called the __ __. | Octet Rule |
| Elements on the right side of the periodic table more right to the next __ __. | noble gas |
| Elements on the left side of the periodic table move __ to the noble gas of the previous row. | backward |
| Atoms will __, __, or __ electrons in chemical reactions to attain this more stable energy state. | gain, lose, or share |
| Elements in families (or groups) other than the noble gases are more __. | reactive |
| A stable electron configuration is called the __ __ configuration. | noble gas |
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IsaacJ
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