Periodic Table Review A – Flashcards
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includes all forms of energy that travel through space in the form of waves |
electromagnetic spectrum |
refers to the distance between two adjacent waves |
wavelength |
numerical value for the speed of all electromagnetic radiation |
3 x 108 m/s |
the number of waves that pass a given point in a specific time |
frequency |
color of light having the shortest wavelength |
violet |
color of light having the longest wavelength |
red |
formula that relates wavelength and frequency |
c = wl x freq |
proportional relationship between wavelength and frequency |
inversely proportional |
proportional relationship between energy and frequency |
directly proportional |
term for lowest energy state of electrons in an atoms |
ground state |
emission of light from metals that have absorbed energy |
photoelectric effect |
formula that relates energy to frequency |
E = hv |
numerical value of Planck's constant |
; ; 6.626 X 10-34 J . s |
; ; ;any energy state of an atom higher than ground state |
; ; excited state |
; ; unit used to measure frequency of light |
; ; ; 1/s or hertz (Hz) |
; ; ; an electron moving from ground state to the excited state must _____ energy |
; ; absorb |
; ; an electron moving from a higher to lower energy;state;must _____ energy |
; ; emit energy |
; ; effect that supports the particle nature of light |
; ; photoelectric effect |
; ; produced by electrons, this supports the wavelike nature of particles |
; ; diffraction pattern |
; ; states it is impossible to simultaneously determine the velocity and position of an electron |
; ; Heisenberg Uncertainty Principle |
; ; he is developed the "planetary model" ;of the atom |
; ; Bohr |
; ; a 3-dimensional region around the nucleus that represents the most probable location of the electron |
; ; orbital |
; ; ; he developed the first periodic table based upon atomic number |
; ; Moseley |
; ; ; he developed the first periodic table based upon atomic mass; |
; Mendeleev |
; ; ; spherical orbital located in each energy level |
; ; ; s |
; ; ; set of dumbbell shaped orbitals located on the x, y, and z axis |
; ; p |
; ; principle that states electrons occupy the lowest energy orbital first |
; ; Aufbau principle |
; ; states that electrons fill orbitals of equal energy before a second electron is added |
; ; Hund's Rule |
groups on the periodic table make up the s-block |
groups 1 and 2 |
groups on the periodic table that make up the p-block |
13-18 |
groups on the periodic table that make up the d-block
|
3-12 |
type of elements located mostly in the s, d, and f blocks |
metals |
blocks referred to as the main-group elements |
s and p |
elements that have properties of metals and nonmetals |
metalloids |
types of orbitals that occupy the 4th energy level |
s, p, d, f |
name for the elements in groups 3-12 |
transition elements |
name for the elements with atomic numbers 58-71 |
lanthanide series |
name for the elements with atomic numbers 90-103 |
actinide series |
most reactive family of metals |
alkali metals |
most reactive family of nonmetals |
halogens |
least reactive family of elements |
noble gases |
block on the periodic table containing the nonmetals |
p |
term for electrons in the outermost energy level |
valence electrons |
term for 8 electrons in the outermost energy level |
octet |
term for elements that make up the f-block |
rare earth elements or inner transition elements |
how to determine the number of valence electrons in groups 13-18 |
subtract 10 from the group number |
term for (+) ions and the type of element that forms them |
cation; metals |
term for (-) ions and the type of element that forms them |
anion; nonmetals |
family name for group 1 |
alkali metals |
family name for group 2 |
alkaline earth metals |