Unit 3: atoms and the periodic chart Flashcards
proton
a positively charged particle in the nucleus
symbol: p+
neutron
a neutral particle (has no charge) in the nucleus
symbol: n0
electron
a negatively charged “particle” outside the nucleus
(actually more of a wave than a particle)
symbol: e-
ion
a charged atom or molecule
Examples: Na+, OH-, Al+3
cation
a positively charged atom or molecule
Examples: Na+, NH4+
anion
a negatively charged atom or molecule
Examples: Cl-, SO4-2
isotope
one type (weight) of an element
A difference in the number of neutrons
Examples: carbon-12 and carbon-14
atomic mass
a weighted average of the naturally occurring isotopes of an element
the bigger number on the periodic chart, with decimals
protons + # neutrons = atomic mass
How do you find the number of electrons?
find the atomic number and adjust for the charge
Example: F-
atomic number 9 + 1 extra electron = 10 e-
atomic number
the number of protons
the smaller number on the periodic chart
a whole number
How do you find the number of protons?
Look at the element’s atomic number.
How do you find the number of neutrons?
Subtract the atomic number from the atomic mass.
Rutherford’s experiment
Shot alpha particles (helium nuclei) at a thin piece of gold foil. Some particles went straight through, others were deflected. Demonstrated that atoms are mostly empty space with a dense core (nucleus). Disproved the plum pudding model.
Bohr’s experiment
He electrified hydrogen gas until it glowed then separated the light with a prism. Demonstrated that there are particular wavelengths of light being given off, which is characteristic of the element. The atomic spectrum shows how much energy is released by the excited electrons falling back down to the ground state.
Which atom has the larger atomic radius, Ca or Ca+2?
Ca
They have the same number of protons. Ca has two more electrons, which makes its electron cloud larger.
Which atom has the larger atomic radius, F- or Na+?
F- They have the same number of electrons (10).
F has 9 protons and Na has 11. More protons pull in the electron cloud more, which makes Na+ the smaller atom.
alpha decay
A radioactive atom breaks apart into two atoms, a helium nucleus (2 protons and 2 neutrons) and the left overs.
beta decay
A radioactive atom breaks apart into an atom and an electron. One of the neutrons splits into a proton and an electron.
4 sources of the elements
1-4 Big Bang
5-26 stellar fusion (the star’s life)
27-92 super nova (star death)
93+ man made
alkali metals
first column
+1 charge
float
react with water
form bases
alkali earth metals
second column
+2 charge
not as reactive as alkali metals
transition metals
middle of the periodic chart
very stable (gold, silver, copper)
bright colors (sapphire, ruby, emerald, paint, etc)
can be +1, +2, or +3 charges
metals
low electronegativity
good conductors of heat and electricity
malleable and ductile
form cations
nonmetals
high electronegativity
gasses or brittle solids
poor conductors
form anions
hallogens
7th column
-1 charge
very reactive
tend to form acids
diatomic (F2, Cl2, Br2, I2)
Noble gases
8th column
no charge
completely stable; don’t react with anything
full s and p orbitals
energy level
the row number
valence electrons
the electrons in the outer energy level
same number as the column number
shown as dots around the symbol in a Lewis Dot Diagram
electron configuration
A list of where the electrons reside in the electron cloud. Can be abbreviated using the nearest noble gas.
quantum numbers
the 4 variables which define an orbital: n, l, ml, ms
The numbers are inserted into equations and graphed. The 3D graph shows the space where the electron is most likely to be found (the orbital).
orbital
the region of space where an electron is likely to be found
Each orbital can hold two electrons (of opposite spin)
s orbital
spherical
there is a single s orbital at every energy level
p orbital
dumbell shaped
there are 3 p orbitals at every energy level except the first level
d orbital
various shapes, including clover leaf
there are 5 d orbitals in the 3rd energy level and at all the higher energy levels
f orbital
various shapes
4th energy level and above
there are 7 different f orbitals
s block elements
Alkali metals and Alkali Earth metals
p block elements
columns 3-8
includes all the nonmetals
d block elements
the transition metals
because of the d orbitals, these elements have more than one stable charge
Ex: Fe+2 and Fe+3
f block elements
lanthanides and actinides (bottom two rows of periodic chart)