Unit 2 Intro Worksheet - Coral Gables Senior High
... 2. Why are you unable to observe the wavelike motion of a soccer ball as it is kicked toward a goal?
3. What is the quantum mechanical model?
4. Explain what is meant by the Heisenberg uncertainty principle.
5. Explain the three principles that govern the electron configuration in an atom.
Periodic Table Puzzle
... Each of the following eight groups has elements with the same number of valence electrons:
Z R D
Chapter 2 Learning Objectives
... 2. Be able to explain the data observed in the photoelectric effect, including:
a. The threshold frequency
b. The correlation between radiant intensity and the number of emitted electrons
3. Understand that the electrons of an atom behave as waves, resulting in quantum numbers
4. Know all four quant ...
09 Exam 1 Key
... 1. (24)a. Number the following types of light from lowest (#1) to highest (#4) frequency.
... The atomic number, Z, equals the number of
protons in the nucleus.
The neutron number, N, is the number of
neutrons in the nucleus.
The mass number, A, is the number of nucleons
in the nucleus.
“Nucleon” is a generic term used to refer to
either a proton or a neutron.
The mass number is not th ...
Chap 2 Solns
... 2.4 (a) Two important quantum-mechanical concepts associated with the Bohr model of the atom are (1) that
electrons are particles moving in discrete orbitals, and (2) electron energy is quantized into shells.
(b) Two important refinements resulting from the wave-mechanical atomic model are (1) that ...
Modern Physics Important Concepts for AP Test
... o E = hf = (hc)/λ
o p = E/c = h/ λ
Matter equations (Matter does not move at c, do not use c = λּ f)
o deBroglie Wavelength λ = h/p = h/(mv) (Common problem on exam)
o f = E/h frequency of matter waves
Davisson Germer Experiment measured wavelength of electrons. (wave
properties of matter)
o Fir ...
... Choose the term from the following list that best matches each description.
Pauli exclusion principle
... which the electrons orbit the nucleus in
accordance with Newton’s Laws but do not
an atom emits or absorbs energy only
when an electron moves from one stable
state to another
Prentice Hall Chemistry Worksheets
... 1. The lowest-energy arrangement of electrons in a subshell is obtained by putting
electrons into separate orbitals of the subshell before pairing electrons.
An atom is the smallest constituent unit of ordinary matter that has the properties of a chemical element. Every solid, liquid, gas, and plasma is made up of neutral or ionized atoms. Atoms are very small; typical sizes are around 100 pm (a ten-billionth of a meter, in the short scale). However, atoms do not have well defined boundaries, and there are different ways to define their size which give different but close values.Atoms are small enough that classical physics give noticeably incorrect results. Through the development of physics, atomic models have incorporated quantum principles to better explain and predict the behavior.Every atom is composed of a nucleus and one or more electrons bound to the nucleus. The nucleus is made of one or more protons and typically a similar number of neutrons (none in hydrogen-1). Protons and neutrons are called nucleons. Over 99.94% of the atom's mass is in the nucleus. The protons have a positive electric charge, the electrons have a negative electric charge, and the neutrons have no electric charge. If the number of protons and electrons are equal, that atom is electrically neutral. If an atom has more or fewer electrons than protons, then it has an overall negative or positive charge, respectively, and it is called an ion.Electrons of an atom are attracted to the protons in an atomic nucleus by this electromagnetic force. The protons and neutrons in the nucleus are attracted to each other by a different force, the nuclear force, which is usually stronger than the electromagnetic force repelling the positively charged protons from one another. Under certain circumstances the repelling electromagnetic force becomes stronger than the nuclear force, and nucleons can be ejected from the nucleus, leaving behind a different element: nuclear decay resulting in nuclear transmutation.The number of protons in the nucleus defines to what chemical element the atom belongs: for example, all copper atoms contain 29 protons. The number of neutrons defines the isotope of the element. The number of electrons influences the magnetic properties of an atom. Atoms can attach to one or more other atoms by chemical bonds to form chemical compounds such as molecules. The ability of atoms to associate and dissociate is responsible for most of the physical changes observed in nature, and is the subject of the discipline of chemistry.Not all the matter of the universe is composed of atoms. Dark matter comprises more of the Universe than matter, and is composed not of atoms, but of particles of a currently unknown type.