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Chapter 3: atoms
This is a review over chapter three in the Physical Science 6th edition textbook
Question/Term | Answer/definition | ||||
---|---|---|---|---|---|
Subatomic particles | Particles that are smaller than atoms, which themselves were once thought to be the smallest possible bits of matter. | ||||
Who were the first to discover atoms | The Ancient Greeks first found atoms, and believed they were invisible. They were first called "atomos," greek word for invisible, but later called atoms. | ||||
John Dalton | Said elements are made of atoms. | Said atoms are indivisible and cannot be destroyed | said the atoms of an element are all alike. | said the atoms of one element are different from the atoms of all other elements, especially their masses. | said the atoms combine chemically in small, whole number ratios. |
Law of electrostatic charges | Opposite electrical charges attract each other, while same charges repel each other. | ||||
JJ Thomson | Used Crookes tubes | Discovered electrons and figured out these particles had a mass, and were not in fact invisible | Developed the plum pudding model | ||
Explain the plum pudding model | This model suggested that negatively charged electrons were embedded in a positive substance. | ||||
Hantaro Nagaoka | Developed the Saturnian model | Thought that the plumb pudding model was faulted in the notion that the opposite electrical charges could mix in the manner the model suggested. | |||
Explain the Saturnian model | This atomic model had a massive and positively charged center surrounded by a flat ring of electrons | ||||
Ernest Rutherford | Believed that a heavy fast-moving particle called an alpha particle directed at an atom should be able to easily pass through it with little or no deflection. | Was surprised to find few of the alpha particles deflected away from the gold foil at very sharp angles in his experiment. | Discovered the nucleus | Developed the nuclear model | |
Explain the nuclear model | Contained a tiny, but massive, positively charged nucleus surrounded by electrons. | ||||
Define quantum mechanics | A branch of physics that explored the behavior of matter and energy at the atomic and subatomic levels. | ||||
Niels Bohr | Used the emission spectrum to go against Rutherford's nuclear model | Stated electrons can only move in distinct energy levels. | Developed the Bohr model | ||
Explain the bohr model | Placed electrons in orbits at specific distances from the nucleus | ||||
Explain the quantum-mechanics model | The oddly shaped, overlapping orbitals of this model indicate areas where electrons in different energy levels are likely to be found. | ||||
Following Ernest Rutherford's discovery of the atomic nucleus, what aspect of an atom's structure were scientists primarily trying to disern? | How electrons move within atoms | ||||
Atoms are made of three basic particles: | electrons | protons | neutrons | ||
Define electron | the smallest of the main subatomic particles, having a mass of 9.1094 x 10^-31kg | ||||
Define proton | a subatomic particle located in the atoms nucleus and has a mass of 1.6726 x 10^-27kg | ||||
Define neutron | a subatomic particle found in the nucleus, but carries no atomic charge | ||||
Define atomic number | The unique number of protons in the atoms of each element | ||||
neutral atom | an atom with balanced electric charges | ||||
Atomic mass | The weighted average of the masses of all the naturally occurring isotopes of that element | ||||
isotopes | The atoms of the same element with differing numbers of neutrons | ||||
isotope name | The unique identifier consisting of each isotope of carbon's name, followed by a number. | ||||
mass number | The total number of particles in it's nucleus | ||||
isotope notation | a X z | ||||
ions | charged atoms with unequal number of protons and electrons | ||||
anions | ions that have more electrons than protons have an excess of negative charge | ||||
cations | ions that have more protons than electrons have an excess of positive charge | ||||
radiocarbon dating | a method of dating geological or archeological specimens by determining the relative proportions of particular radioactive isotopes present in a sample. |