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Atoms, Elements and Periodic Table Quiz
Study Guide
1. Atom concept—origins—Democritus and Aristotle in ancient Greece
2. John Dalton—first published atomic theory, proposed each element has a particular
structure of atom.
3. J. J. Thomson—cathode ray tube experiment, discovered electron, plum pudding
model of atom
4. Ernest Rutherford—gold foil experiment, discovered nucleus, positive charges to
particles like protons.
5. Niels Bohr—first proposed electrons moving in energy levels. Designed the first
working model of an atom with electrons.
6. Modern Atomic Theory—electron cloud model, the atom is the smallest part of an
element that has the same properties as that element. Atoms are composed of protons,
neutrons and electrons. Electrons move in clouds of orbitals in energy levels outside
nucleus.
7. nucleus—contains protons and neutrons
8. protons—positive charged particles in nucleus
9. neutrons—neutral (no charged) particles in nucleus
10. electrons—negatively charged particles that follow orbitals around nucleus.
11. atomic number—the number of protons in an atom of an element
12. mass number—the average of the abundance of the isotopes of atoms of an
element (contains both protons and neutrons).
13. isotope—an atom of an element with a different number of neutrons.
14. ion—an atom with a charge due to a different number of electrons.
15. orbital—a three dimensional shaped path that electrons follow when moving around
the nucleus. Different shells of electrons contain different numbers and shapes of these
orbitals. The orbitals are labeled s, p, d and f.
16. Forces in atoms: four forces are at work in all matter: gravitational force,
electromagnetic force, strong nuclear force, and weak nuclear force.
17. Gravitational force—between anything with mass, very small in atoms.
18. Electromagnetic force—attraction between opposite charges keeps electrons
bound to nucleus of atoms. Without it, we would not have atoms.
19. Strong force—between larger particles when close together—overcomes the
repulsive electromagnetic force between protons in nucleus to hold the nucleus
together—without it, we would not have any atoms.
20. Weak force—between particles that can decay and become other particles. Without
it, radiation would not work and energy could not be exchanged between particles, thus,
no atoms.
21. Dmitri Mendeleev—Russian chemist who first conceived of the Periodic Table of
Elements.
22. Periodic Table of Elements—an arrangement of elements by increasing atomic
number and by similar properties based on their VALENCE. Using this table, the metals
are on the left, the non-metals on the right, divided by a stair step line which contains
the metalloids (between metals and non-metals).
23. Metals—give up electrons-good conductors.
24. Non-metals—accept electrons—good insulators.
25. Metalloids—in between—semi conductors—make good materials for digital
devices. (Like Silicon).
26. Periods—rows of the Periodic Table that correspond to the filling of a particular
electron shell.
27. Family/Group—a column of the Periodic Table that includes elements with the
same VALENCE, thus making them interact in similar ways with other elements
(combine into similar compounds.) The maximum number of electrons in a shell
typically increases with distance away from the nucleus of the atom. The Valence
repeats in a periodic pattern, thus we have a “Periodic” Table of elements.
28. Unusual elements—Hydrogen and Helium can react differently from other elements
due to their small size and different structure, thus they are often removed from the
other part of the table and set apart.
29. Valence—the number of electrons in the outer shell of an atom of an element. It
determines how an atom will interact with other atoms.
30. Atom stability—atoms want to be stable and balanced—they prefer to have either a
full or empty outer shell of electrons.
31. Valence and Family of Elements—Each family of elements has a particular valence
number that determines its reactivity with other elements.
32. Alkali Metals—Group 1 metals that have a high reactivity, and can explode violently
when reacted with water or other substances.
32. Alkaline Earth Metals—Group 2 metals that are reactive, and tend to bond with two
elements or in double bonds.
33. Halogens—Group 17 non-metals that like to bond with the Alkali Metals to form
compounds. They are good insulators.
34. Inert (Noble) Gases—Group 18 elements that tend to not react much due to their full
outer shells of electrons. Includes Helium, Neon, Krypton, etc. used in advertising signs.
35. Transition Metals—the middle groups 3-11 in the Periodic Table including copper,
gold, silver, zinc, etc. They can form multiple bonds and sometimes have two unhappy
outer shells of electrons. They often combine into alloys of two or more metals together
(examples—gold and silver jewelry.)