Science Test (Chapter 18) Flashcards
Chemical Symbol
Is a short or abbreviated name of an element.
List the 6 ways scientists determine shorthand for element names. Examples for each.
The 6 ways scientists determine shorthand for element names are: 1. Derived from Latin- Ex: Argentum is Latin for silver = Ag.
2. Honoring scientists (people)- Ex: Curium was named to honor Pierre and Marie Curie who researched radioactivity = Cm
3. Honoring places- Ex: Germaniums was named after Germany = Ge
4. Honoring their properties- Ex: Cesium was discovered by Robert Bunsen (inventor of the Bunsen burner) and because the element imparts a blue color, Bunsen named it cesium from the Latin word caesius, meaning, “sky blue” = Cs
5. First letter of the element- Ex: oxygen
6. First letter of the element and another letter in the name/word. Ex: Calcium = Ca (3L’s 3P’s)
Create a chart comparing protons, neutrons, and electrons. Be sure to address charge, location, and composition.
Protons: Positively Charged 1+, located in the nucleus, are made up of 3 quarks.
Neutrons: Have no charge- Neutral, located in the nucleus, are made up of 3 quarks.
Electrons: Negatively charged particles 1-, occupy the space surrounding the nucleus in an electron cloud/are orbiting around the nucleus, and its composition is unknown.
The model of the atom has changed over time. As scientists performed experiments and learned more about the structure of the atom, the model was modified. Describe how the atomic model has changed over time to become what it is today and clarify which model we use today. Use details to support your answer.
The atomic model has changed over time because each time scientists have discovered different components (more subatomic particles). The model has evolved from Democritus’ uncuttable atom, the Thomson Model which is a ball of positive charge with negatively charged electrons, to the Rutherford Model “empty space with electrons” with the positively charged ball in the center, the Bohr Model with a nucleus made up of protons and neutrons, as well as electrons in space, lastly, the Electron cloud model that we currently use today containing electrons that do not follow fixed orbits, but tend to occur around the nucleus.
How were quarks discovered? How many are there and what were they called? Why was the 6th quark difficult to find?
Quarks were discovered by the machines of the Tevatron located in Ilinois and the Large Hardon Collider in Switzerland. These machines helped scientists learned that quarks exist by accelerating charged particles, so they could study the tracks after they collided/These machines accelerate charged particles to tremendous speeds and then force them to collide and smash into protons, causing the protons to break apart. They then study the tracks that different particles leave behind. (There are 6 different types of quarks.) (The top, bottom, down, up, charm, and strange). The 6th quark was difficult to find because only about one billionth of a percent of the proton collisions performed showed the presence of them. (SHOWS WHY THEORIES ARE SO IMPORTANT)
What are two similarities of protons and neutrons?
Protons and neutrons have the same mass and are both located in the nucleus.
What is the relationship between protons and the nucleus?
The relationship between protons and the nucleus is that protons make up the nucleus and they are the reason the nucleus is positive.
What is wrong with these element symbols: CA, mg, aT?
- The a is capitalized.
- The m is not capitalized.
- The t should not be capitalized and the a should be capitalized.
How should these symbols be written: CA, mg, aT?
- Ca
- Mg
- At
Why are most atoms neutral? Ex.
Most atoms are neutral because they have the same number of protons and electrons, cancel each other out positive and negative. Ex, -1+1=0
Are electrons, protons, or neutrons the smallest particles? If not, what are? How do you know?
Electrons, protons, or neutrons are not the smallest particles because quarks are!! I know because quarks are the tiniest subatomic particles that make up protons and neutrons.
Label the atomic models from progression over the years and label the parts of an atom!
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Nucleus
Small, positively charged center of the atom.
Protons
Positively charged particles located in the nucleus.
Neutrons
Electrically neutral particles that are located in the nucleus, that have no charge.
Electrons
Negatively charged particles that occupy the space surrounding the nucleus in an electron cloud.
Quarks
Smaller particles that make up only protons and neutrons.
Atom
An atom is the smallest particle of an element that retains the elements’ properties/characteristics.
How many different charges are there in an atom and what are they?
Two. Positive protons and negative electrons.
What are the four subatomic particles that make up an atom?
Protons, neutrons, electrons, and quarks.
Why do you think the nucleus of an atom is positively charged?
The nucleus of an atom is positively charged because it contains protons that are positive and neutrons that have no charge. So all of the charge is positive.
Where is most of the mass in an atom found? Why is that?
Most of the mass is found in the nucleus because it is made up of protons and neutrons that are equal to about 1amu, while an electrons’ mass is so light it is considered to be negligible.
What is the difference between the atomic number and the atomic mass? What is the similarity?
The difference between atomic number and atomic mass is that atomic number is the number of protons in the nucleus of an atom or atom of the element. Whereas, (average) atomic mass is the weighted-average mass of the mixture of its isotopes. The similarities are that they are both on the periodic table of elements and they both relate per element- means every element has. (Atomic Number and Atomic Mass) The whole element relates to both of them.
Describe the relationship between isotopes and average atomic mass. Ex.
The relationship between Isotopes and average atomic mass is that isotopes, the same element with different numbers of neutrons, make us have different mass numbers that forces you to take an average. (Isotopes make/made us need an average atomic mass)
Isotopes (neutrons)- different mass numbers- average atomic mass.
Grades (in school)- different grades- average grade- shows a general idea of how everyone did.
How can you determine:
-the atomic number of an element
-the number of protons an element has
-the number of neutrons an element has
-the mass number of an element
- You can determine the atomic number of an element by counting, the number on the periodic table of elements, and the same as protons.
- You can determine the number of protons an element has because it is the exact same number as the atomic number and the electrons, if neutral or if you have the mass number and the number of neutrons you can subtract them to get the number of protons.
- You can determine the number of neutrons there are by subtracting the mass number and the atomic number or the number of protons to get the number of neutrons.
- You get the mass number of an element by adding the number of neutrons and the number of protons or the atomic number per atom.
Atomic number and example.
The number of protons in an atom of an element is equal to a number called the atomic number or the number of protons in an atom’s nucleus. Ex, the atomic number of carbon is six. (Means six protons)
Mass Number and example
(Of an atom) is the sum of the number of protons and the number of neutrons in the nucleus of an atom. For example, carbon with a mass number equal to 12, or carbon-12, is the most common form of carbon.
Isotopes and example
Atoms of the same element with different numbers of neutrons. Ex, you have the element boron and the naturally occurring atoms of boron have mass numbers of 10 or 11. (Different numbers of neutrons) SAME NUMBERS OF PROTONS, OTHERWISE IT IS A DIFFERENT ELEMENT!
Average atomic mass and example.
(Of an element) is the weighted-average mass of the mixture of its isotopes. Ex, the atomic mass of boron is 10.8 amu- atomic mass unit.
What are the similarities between atomic mass and mass number?
The similarities between atomic mass and mass number are that they both include protons and neutrons and are the weight of atoms in an element.
What are the similarities between atomic number and mass number?
The similarities between atomic number and mass number are that to get both of them you have to count particles, are both accurate numbers (not decimals), and relate to a specific atom.
What are the similarities between atomic mass, mass number, and atomic number?
The similarities between atomic mass, mass number, and atomic number are that they are all numbers, all include protons, and are all atoms of elements.
Practice diagrams of isotopes.
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What can you compare isotopes to?
You can compare isotopes to apples because they all look and taste the same, and they are the same size- still apples, much like isotopes because they are the same element. But they may not be the same inside. If you cut open an apple, you will see the seeds at the core.
