Name: ___________________________________ Date



Name: ___________________________________ Date: ___________________________ Period: ______

Interactive Textbook Activity – Physical Science

Chapters 4 : Atoms and the Periodic Table

Directions: Access your HRW account on the Holt McDougal website ( ) and log in with your personal username and password). Click “Go to the online textbook.” Using the drop down menu on the top of the page select Chapter 4: Atoms & the Periodic Table, then click “Go.” Click on the visual concepts tab at the top. Watch each of the Visual Concepts multimedia presentations and answer the following questions.

Section 1 Atomic Structure

Atom

1. An atom is the ________________ unit of an __________________ that maintains the properties of that __________________.

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Parts of an Atom

1. The electron _____________is the region surrounding the ______________ of an atom where electrons are ______________ to be found. 

2. The Nucleus is the ____________________ charged, center it contains most of the atoms ______________________.

3. The electrons are _________________ charged found in the electron ___________, the size of the electron cloud ___________________ the size of the atom.

4. Protons are the __________________ parts of an atom.

5. The particle with no charge in the nucleus is the ___________________.

6. What happens to the neutrons colors when you scroll/put curser on them? ___________________________________________________________________

Bohr’s model of the Atom

1. ________________ Bohr suggested that electrons in an atom move in set _____________ around the nucleus, much as the _________________ orbit the _______ in our solar system.

2. In Bohr's model, each _______________ has a certain ________________ that is determined by its path around the nucleus. Electrons can be only in _____________ energy levels and must __________ or ________________ energy to change ________________.

3. In the late _________________ scientist noticed a __________________ color light was produced when high ___________ electric current was put through hydrogen gas.

4. What is emitted when an electron falls downward to a lower energy level orbit? ______________________________________

Electron energy levels

1. The ________________ of electrons in an atom can take on only certain _____________, or "levels," and in a given atom, there are a __________ number of electrons that can occupy any particular energy _________________________.

2. Just as guests in a _________________ cannot stay "between" ________________, electrons in an atom must occupy a given energy level. Hotels have a set number of rooms on each floor. Similarly, there is a ____________________ number of electrons that an atom can hold at each energy level. 

3. What is the name of the motel : ___________________ (in the model diagram shown) 

4. Where is the nucleus in our model ? _________________________

5. The second energy level can hold how many electrons? __________________

.

Comparing models of atoms

1. Significant models of atoms include those of: 3 people which are:

• Thomson

• _______________________

• _______________________

2. Thomson discovered the _______________________ and proposed the ___________________ model. That held electrons in a _________________ charged sphere like shape.

3. Rutherford discovered that atoms where mostly ________________ ________________ and also discovered the center of the atom the _______________________.

4. Borh’s model explain how electrons move around the _____________ and why atoms could only absorb or give off certain amounts of _______________________.

5. Electrons today are not ____________ particles and are found in regions of high ___________________________ areas around the nucleus.

Orbital

1. An orbital is a ___________ - ________________ region around the nucleus that indicates the probable location of an electron. 

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s-Orbital

1. When the angular momentum _______________ number equals 0, the electrons are in the s–orbital. These orbitals are ______________________ and are the first orbitals occupied at a given energy level. An s–orbital has only one possible orientation and can hold up to _______ electrons.

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p-Orbital

1. When the _______________ momentum quantum number equals 1, electrons are in the p–orbital. These orbitals resemble a very full _________________ pinched in the middle and are filled after the s–orbitals are filled. A p–orbital has 3 possible ____________________, each of which can hold ________ electrons. Which makes a total number of electrons = ________.

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Valence electrons

1. A valence electron is an electron that is _________________ to be lost, gained, or ___________ in the formation of __________________ compounds. .

2. These electrons are found in the _____________________ energy level of an atom.

3. Oxygen has ________ valence, Sodium has __________, The noble gas Neon has __________ and the outer most orbital is completely ______________.

4. On the periodic table the Alkali-earth metals have _______ valence electrons and the nitrogen group has __________ valence electrons.

Section 2 Guided tour of the periodic table

Periodic table overview

1. The periodic table ________________ the different types of atoms, or chemical ____________. The elements are arranged by atomic number in _______________and columns, from left to right and top to bottom. Vertical columns are called groups or ______________ of elements while __________________ of elements consist of ___________________ rows.

2. There are __________ elements that occur naturally on the periodic table.

3. _____________ is the simplest element, going up to _______ (symbol) Ununpentium which is the most complex.

4. The table is organized by the number of protons which is the _____________ _____________.

5. The vertical groups are called ________________________.

6. The horizontal rows are called a __________________________.

7. The elements 93 and higher are not very _________________ and are radioactive and ________ rapidly.

Ioniazation

1. Atoms are electrically __________________l; the number of negatively charged electrons is __________________ to the number of positively charged protons.

2. An ion is an atom that has an _________________ charge, either positive or negative. ___________________ is the process whereby gaseous atoms become electrically charged. 

3. If an ion is positively charged it is an _____________ an negatively charged is an _____________

Ion

1. An ion is an atom, __________________, or molecule that has ____________ or lost one or more electrons and has a negative or positive ______________________.

2. What are the two ions shown in this slide section : ________________ and ______________ together they make salt.

Comparing cations to anions

1. Cations are ions that have a _______________charge.

Anions are ions that have a _______________ charge.

Atomic number

1. The atomic number is the number of _________________ in the nucleus of an atom. The atomic number is the same for all _______________ of an element. 

2. The atomic number for oxygen is ____________________

3. What is its’ electron configuration shown that is abbreviated? ____________________________

Atomic mass

1. The mass number is the sum of the numbers of protons and _____________ in the nucleus of an atom. Because electrons have very _______________ mass, the mass number is very close to the average atomic mass of the element.

2. What is the atomic mass of oxygen(write out whole number) : _______________________

Isotopes and Nuclides

1. Isotopes are atoms of the same element that have different _____________________.

2. Nuclide is the general term for any __________________ of any element, based on the number of protons and neutrons in its ____________________. 

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Average atomic mass

1. The average atomic mass is the _________________ ________________ of the atomic masses of the naturally occurring ______________________of an element. 

2. Elements can have more the _____________ stable isotopes.

3. Copper is made up of two stable isotopes which are ____________ and ____________, which is ______________________ grams per mole.

Section 3 Famlies of elements

Comparing metal, nonmetals and metaliods

1. Metals

- are good _____________ of heat and electricity

- have a _________ surface appearance

- are easy to form and __________

2. Nonmetals

• are ______________ conductors of heat and electricity

• have a ____________surface appearance

• are very ____________________

3. Metalloids

• have some characteristics of ___________ and some characteristics of nonmetals

• are ______________________ (conducting electricity only at high temperatures)

• _______________ have either a _____________, metallic surface appearance or a ______________, nonmetallic surface appearance

• are usually more _______________ than metals but are easier to ___________ and form than nonmetals

Sec. 4 Using moles to count atoms

The mole

1. A mole is the _________________ of a substance that contains as many particles as there are atoms in exactly _______ g of ___________________–12.

2. 1 mole = ________________________________ atoms of a material.

3. True or False – a mole of iron and a mole of copper have the same mass.

Avogadro’s number

1. The number of _______________________ in 1 mole equals 6.022 x 1023 per mole. 

2. If we covered the USA with a mole of popcorn it would be __________ km high or thick and would be twice as high as the ________________ _________________ station. 

3. A mole of magnesium would weigh _______________________ grams.

Molar mass

1. A mole of any other kind of atom or molecule will _______________ contain the same number of particles 6.02 x 1023 particles. The mass, however, will ___________ , because the particles have different ________________. Molar mass is the mass in ___________ of one mole of a substance. 

2. A molar mass of iron equals _____________________.

Conversion factor

1. Boyle's law states that the ______________ of a fixed mass of gas varies _________________ with pressure at constant _____________________. As the volume _____________________, the pressure _________________________. As the ________________ decreases, the ___________________ increases. . 

Dalton’s Law of Partial pressure

1. A conversion factor is a _________________ derived from the equality between two different ________________ that can be used to convert from one unit to the other. 

2. 3 dozen eggs = ______________________ eggs. 

3. 0.5 moles of silver = _______________________________ atoms of silver.

Concept map

The number of

In an atom is called in the

An determining where of an atom is the

Is located in the which is different

For each

Which is classified into

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