Show:
The Atom
Atomic Emission Spectra
Subatomic Particles 1
Subatomic Particles 2
Pot Pourri
100
True or False: The nucleus takes up most of the atom
False
100
When an atom gains energy, what happens to the electrons?
Move to higher energy levels
100
the atomic number is always equal to the number of _________
protons
100
What is the charge of a proton?
+1
100
The smallest building block of matter is called the ______
atom
200
The mass # of an atom is equal to ___________
Protons + neutrons
200
True or False: The atomic emission spectra is the same for H and Li because they are in the same column on the Periodic Table. WHY?
False--every element has a unique emission spectrum
200
What is the mass of a proton?
1 amu
200
What is the mass of a neutron?
1 amu
200
The first energy level in Bohr's model holds ______ e-
2
300
Every oxygen atom has what in common?
# protons
300
What causes each line in the spectrum?
An electron giving off energy as it drops to a lower energy level
300
What is the charge of an electron?
-1
300
What is the charge of a neutron?
0
300
The second energy level of Bohr's model holds _____ e-
8
400
The ____________is when all of the electrons are in the lowest possible energy level.
ground state
400
What do you use atomic emission spectra for?
Identifying what things are made of.
400
Where do you find neutrons in an atom?
In the nucleus
400
Where do you find electrons in the atom?
Outside the nucleus--in the electron cloud
400
True or False: The electron cloud model tells exactly where the electrons are.
False--most likely location
500
To become a negative ion, the atom gains ________
electrons
500
When an electron drops to lower energy levels, what happens to the energy?
released as a photon of light.
500
What is the mass of an electron?
0 amu
500
If you have the mass # and the atomic #, how do you find the number of neutrons?
subtract at# from Mass#
500
Carbon-12 and Carbon 13 have a different number of __________
neutrons