Download study guide: subatomic particles test

32. How does the charge of the nucleus differ from the charge of the
entire atom? The nucleus always has a positive charge—The charge
of the entire atom is usually zero (because A=P=E) unless we have an
ion—in which case we would be told.
33. What can cause an atom to be an ion? When, during a reaction, the
number of electrons changes and the number of protons and
electrons are no longer equal —How do we calculate ionic charge?
Count the number of protons and count the number of electrons,
finding the difference between the two and assigning the charge
(either positive (+) or negative (-) based on which particle there is
more of (more protons = positive, more electrons = negative charge).
What subatomic particles is it based on? Protons and electrons —
Explain. Protons and electrons are the only particles in the atom
with a charge.
34. What do Bohr Models show?—Explain. All electrons on their specific
energy levels
35. What is the maximum number of electrons that can fit on each of the
first three energy levels in a Bohr Model?
1st—Holds up to 2
2nd—Holds up to 8
3rd—Holds up to 18
36. What is a major limitation of a Bohr Model? They do not always
accurately show valence electrons—most of the time they do, but if
the number of electrons in the outer shell is more than 8, you must
consult the Periodic Table and follow our rules:
Group 1: 1 valence electron
Group 2: 2 valence electrons
Groups 13-18: Have 3, 4, 5, 6, 7, or 8 (subtract 10 from group
number)
STUDY GUIDE: SUBATOMIC PARTICLES TEST
ATOMS REVIEW:
1. Atoms are composed of three main parts, called subatomic particles:
the protons, neutrons, and electrons.
2. Most of the mass of the atom is concentrated in the nucleus of the
atom due to this being the location of the protons and neutrons.
3. The sum of the number of protons and neutrons in a particular atom
is called the mass number.
4. Valence electrons are the outermost electrons in an atom. They
determine an atom’s reactivity and chemical properties.
5. The type of atom (its name) is determined by the number of protons
it contains.
6. The number of protons in an atom is called the atomic number and is
equal to the number of electrons.
MORE PRACTICE:
1. Identify the charge, location, and role the proton plays in the atom.
Positive (+), inside the nucleus, contributes to the atom’s mass and
charge
2. Identify the charge, location, and role the neutron plays in the
atom. Neutral/none (0), inside the nucleus, contributes to the
atom’s mass only
3.
Identify the charge, location, and role the electron plays in the
atom. Negative (-), outside the nucleus, contributes to the atom’s
charge only
4.
How does the mass of protons, neutrons, and electrons compare to
one another? Protons and Neutrons have an equal mass (1 amu);
Electrons are 2000 times smaller (We say they have no mass
because their mass is so insignificant)
5.
How do you find the number of protons that an element contains
using the Periodic Table? A=P=E (Atomic number equals the
number of protons which equals the number of electrons)
6.
7.
8.
9.
How could you determine the number of protons if you were given the
number of electrons? A=P=E (Atomic number equals the number of
protons which equals the number of electrons)
19.
What do we call a charged atom? An ion
20.
What makes an atom have a charge? When, during a reaction, the number of electrons
changes and the number of protons and electrons are no longer equal
How could you determine the number of protons if you were given the
atomic mass and the number of neutrons? M-A=N (Mass minus atomic
number equal the number of neutrons), and A=P=E, so the mass minus
the number of neutrons equals the number of protons.
AND MORE PRACTICE:
21.
What is an atom? Smallest part of an element
How do you find the number of electrons an element contains using the
Periodic Table? A=P=E (Atomic number equals the number of protons
which equals the number of electrons)
How could you determine the number of electrons if you were given the
number of protons? A=P=E (Atomic number equals the number of
protons which equals the number of electrons)
10. How do you find the number of neutrons an element contains? M-A=N
(Mass minus atomic number equal the number of neutrons)
22.
How does the entire diameter of the atom compare to the diameter of the nucleus
alone?—What does this tell us about an atom? The diameter of the entire atom is
~100,000 times bigger than the diameter of the nucleus; Atoms contain a lot of empty
space despite their tiny size.
23.
List the 3 subatomic particles. Protons, neutrons, electrons
24.
Identify the charge, location, and role each subatomic particle plays in the atom.
Protons: Positive (+), inside the nucleus, contributes to the atom’s mass and charge
Neutrons: Neutral/none (0), inside the nucleus, contributes to the atom’s mass only
Electrons: Negative (-), outside the nucleus, contributes to the atom’s charge only
25.
Identify some similarities amongst the 3 subatomic particles, as well as some differences.
Protons and neutrons have the same mass and are both inside the nucleus; Protons and
electrons both have a charge; Protons are the only particles with a charge and mass;
Neutrons are the only particle without a charge; Electrons are the only particle without a
significant mass (so we say it has no mass).
26.
Where is the majority of the atom’s mass concentrated? Inside the nucleus (where the
protons and neutrons are located)
27.
What is the atomic number? The number of protons Where is it located on a Periodic
Table square? Top of the square Which subatomic particle(s) does it involve? Protons
specifically, but A=P=E (so, in a stable, atom, it also equals the electrons)
28.
What is the atomic mass? The number of protons plus neutrons Where is it located on a
Periodic Table square? Bottom of the square Which subatomic particle(s) does it involve?
Protons and neutrons
29.
How do we find the number of protons, neutrons, and electrons an atom contains by
looking at the Periodic Table? (THINK APE MAN) Protons and electrons can be found by
looking at the top of the square (A=P=E); Neutrons can be found by rounding the mass
(bottom of the square) to the nearest whole number and subtracting the atomic number
(top of square from it)—(M-A=N)
30.
What are valence electrons? Electrons in the outermost energy level of an atom—How do
we determine the number of valence electrons an atom contains, by using the Periodic
Table? Group (column) 1 elements have 1 valence electron, Group 2 elements have 2
valence electrons, and groups 13-18 have 3, 4, 5, 6, 7, or 8 (subtract 10 from group
number)—Remember our rules and the exception in Group 18!—Exception is Helium in
group 18 (doesn’t have 8 valence electrons, like the rest of the group, because it only has
2 total electrons)
31.
What gives an element its identity (other than its name or symbol)? The number of
protons it contains
11. What gives an element its identity? Protons
12. How do you find the number of valence electrons an element contains
using the Periodic Table? Group (column) 1 elements have 1 valence
electron, Group 2 elements have 2 valence electrons, and groups 13-18
have 3, 4, 5, 6, 7, or 8 (subtract 10 from group number)
13. If you were given a picture of an atom, how could you determine valence
electrons, without consulting the Periodic Table? Valence electrons are in
the outermost energy level of the atom (Highlight the outer ring and
count the number of electrons present).
14. If you were given a picture of an atom, how could you determine which
element on the Periodic Table the atom represents? Count the number of
protons in the atom’s nucleus and remember A=P=E
15. If you were given a picture of an atom, how could you determine the
atom’s charge? Count the number of protons and count the number of
electrons, finding the difference between the two and assigning the
charge (either positive (+) or negative (-) based on which particle there is
more of (more protons = positive, more electrons = negative charge).
16. If you were given a picture of an atom, how could you determine the
atom’s mass? Add the number of protons to the number of neutrons
(because these are the only 2 particles with mass)
17. Where is most of the mass of the atom concentrated? Nucleus (where
protons and neutrons are located—the only particles with mass)
18. Even though an atom contains 3 subatomic particles, often in large
numbers, the atom still contains a lot of empty space.