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atoms periodic table study guide answerThe current custom error settings for this application prevent the details of the application error from being viewed remotely (for security reasons). It could, however, be viewed by browsers running on the local server machine. It looks like your browser needs updating. For the best experience on Quizlet, please update your browser. Learn More. Electrons A part of a atom that is negative and is found on the outer energy levels of a atom Electron Cloud Electron cloud is used to describe where electrons are when they go around the nucleus of an atom Neutrons A part of a atom that has no charge and is found in the nucleus of a atom. Energy levels A fixed amount of energy Nucleus It's the central part of the atom; it consists of protons and neutrons. It is also surrounded by electrons that are on energy levels. Element Pure substance made of one type of atom Isotope Forms of the same element of the same element with a different number of neutrons Neutral atoms Atoms with an overall charge of 0 What is the basic history of the atomic structure. Used to believe it was a small individual unit What is the most current history of the atom. An atom has a nucleus Quantum Mechanical model Model that uses complex shapes Chemical properties characteristics of a material that becomes evident when there is a reaction Physical properties any property that is measurable, whose value describes a state of a physical system Metals any chemical element that is a good conductor of electricity and heat Non-metals an element or substance of that is not metal Electromagnetic spectrum a continuum of electromagnetic waves arranged according the frequency and wavelength Emission spectrum Releases energy Absorption spectrum Absorbs energy What type of light has the most energy and least frequency. Red What type of light has the least energy and most frequency. Purple The most common carbon atoms have six protons and six neutrons in their nuclei.http://www.misvo.cz/userfiles/electrical-pro-calculator-manual.xml
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What are the atomic number and the mass number of these carbon atoms? The atomic number is 6 and the mass number is 12 An isotope of uranium has an atomic number of 92 and a mass number of 235. What are the number of protons and neutrons in the nucleus of this atom. The proton number is 92 and the neutron number is 143 The number of protons in the nucleus of a tin atom is 50, while the number of neutrons in the nucleus is 68. What are the atomic number and the mass number of this isotope. The atomic number is 50 and the mass number is 118 Explain how atoms are composed. With protons, neutrons, and electrons Which is larger, a proton or an electron.Where is most of the mass of an atom located. Nucleus S orbital holds 2 P orbital holds 6 D orbital holds 10 F orbital holds 14 Atom Smallest unit of ordinary matter How much bigger is an oxygen atom to a hydrogen atom? 8 times bigger Cathode ray a beam of electrons emitted from the cathode of a high-vacuum tube Which orbit has the greatest energy. E6 Which orbit has the least energy. Books Audiobooks Magazines Podcasts Sheet Music Documents (selected) Snapshots Enjoy thousands of titles when you subscribe Read free for 30 days Atoms and The Periodic Table Study Guide Answers Uploaded by api-267855902 100 (1) 100 found this document useful (1 vote) 3K views 10 pages Document Information click to expand document information Description: The number of protons determines the type (identify) of the element. Report this Document Download now Save Save atoms and the periodic table study guide answers For Later Atoms and The Periodic Table Study Guide Answers Original Title: atoms and the periodic table study guide answers Uploaded by api-267855902 100 (1) 100 found this document useful (1 vote) 3K views 10 pages The number of protons determines the type (identify) of the element. What are different forms of the same element called? -isotopes.http://vinovnik.cz/files/electrical-panel-maintenance-manual.xml What happens to the number of valence electrons as you move across the periodic table? -increase. What is a characteristic of an unstable isotope? -radioactive. More Save Save atoms and the periodic table study guide answers For Later 100 100 found this document useful, Mark this document as useful 0 0 found this document not useful, Mark this document as not useful Embed Share Print Download now Jump to Page You are on page 1 of 10 Search inside document. Learn about Easel TOOLS Easel Activities Pre-made digital activities. Add highlights, virtual manipulatives, and more. Browse Easel Activities Easel Assessments Quizzes with auto-grading that will be available for purchase on TpT soon. Some filters moved to Formats filters, which is at the top of the page. This is a great introductory activity to get students familiar with the table. This is one of my best sellers and my all time favorite lesson to teach. Using their own table, students will search for different elements using the group, period, name, symbol, or atomic number. They will be able to explain how properties are used to classify elements. Elements have a data page bulleting information about its facts, uses and discovery. The following page are pictures to color pertaining to those facts. It covers the first 85 elements plus activities at the end. Student answer sheets and teacher answer key are provided. IncludesStudents begin with four input activities where they read articles, explore hands-on demos, research online, and watch videos all about the periodic table. These coloring pages and puzzles are a great way to practice some of these fundamental Chemistry concepts. The atomic theory workbook is found in the BONUS FILE of this bundle. (I had originally bundled some resources prior to making workbooks.) The key is part of that download. The Elements: Metals vs. If your students can remember that the Alkali and Alkaline Earth metals are the 'hippies', they will also remember that these atoms give away their valence electrons.Easy and no prep bulletin board. All you need to do is print on different colored paper- NO COLORED INK REQUIRED! I suggest laminating for extended use and protected storage. Your choice of squares that have atomic ma Subjects: Science, Basic Principles, Chemistry Grades: Not Grade Specific Types: Printables, Bulletin Board Ideas Show more details Add to cart Wish List showing 1 - 24 of 3,893 results 1 2 3 4 5 Next Teachers Pay Teachers is an online marketplace where teachers buy and sell original educational materials. Are you getting the free resources, updates, and special offers we send out every week in our teacher newsletter? Sign Up. Steve Cole, Getty ImagesShe has taught science courses at the high school, college, and graduate levels. The elements couldn't be changed using any chemical method. Each element has a unique number of protons. If you examine samples of iron and silver, you can't tell how many protons the atoms have. However, you can tell the elements apart because they have different properties. You might notice there are more similarities between iron and silver than between iron and oxygen. Could there be a way to organize the elements so you could tell at a glance which ones had similar properties?You can see Mendeleev's original table (1869). This table showed that when the elements were ordered by increasing atomic weight, a pattern appeared where properties of the elements repeated periodically. This periodic table is a chart that groups the elements according to their similar properties.Many elements remained to be discovered in Mendeleev's time. The periodic table helped predict the properties of new elements.What do you notice? Mendeleev's table didn't have very many elements, did it. He had question marks and spaces between elements, where he predicted undiscovered elements would fit.When you look at the modern periodic table, do you see any skipped atomic numbers that would be undiscovered elements. New elements today aren't discovered. They are made. You can still use the periodic table to predict the properties of these new elements.Atom size decreases as you move from left to right across the table and increases as you move down a column. The energy required to remove an electron from an atom increases as you move from left to right and decreases as you move down a column. The ability to form a chemical bond increases as you move from left to right and decreases as you move down a column.Why was the table changed. In 1914, Henry Moseley learned you could experimentally determine the atomic numbers of elements. Before that, atomic numbers were just the order of elements based on increasing atomic weight. Once atomic numbers had significance, the periodic table was reorganized.Atomic number increases as you move across a row or period.The period number of an element signifies the highest unexcited energy level for an electron in that element. The number of elements in a period increases as you move down the periodic table because there are more sublevels per level as the energy level of the atom increases.Elements within a group share several common properties. Groups are elements have the same outer electron arrangement. The outer electrons are called valence electrons. Because they have the same number of valence electrons, elements in a group share similar chemical properties. The Roman numerals listed above each group are the usual number of valence electrons. For example, a group VA element will have 5 valence electrons.The group A elements are called the representative elements. The group B elements are the nonrepresentative elements.On many printed periodic tables you can find an element's symbol, atomic number, and atomic weight.The major categories of elements are the metals, nonmetals, and metalloids.Aluminum foil is a metal. Gold and silver are metals. If someone asks you whether an element is a metal, metalloid, or non-metal and you don't know the answer, guess that it's a metal.They are lustrous (shiny), malleable (can be hammered), and are good conductors of heat and electricity. These properties result from the ability to easily move the electrons in the outer shells of metal atoms.There are so many metals, they are divided into groups: alkali metals, alkaline earth metals, and transition metals. The transition metals can be divided into smaller groups, such as the lanthanides and actinides.Sodium and potassium are examples of these elements. Alkali metals form salts and many other compounds. The alkali metals are highly reactive.Calcium and magnesium are examples of alkaline earths. These metals form many compounds. Their atoms are smaller than those of the alkali metals.Iron and gold are examples of transition metals. These elements are very hard, with high melting points and boiling points. The transition metals are good electrical conductors and are very malleable. They form positively charged ions.The lanthanides and actinides are classes of transition elements. Another way to group transition metals is into triads, which are metals with very similar properties, usually found together.Just under iron, cobalt, and nickel is the palladium triad of ruthenium, rhodium, and palladium, while under them is the platinum triad of osmium, iridium, and platinum.The top row has atomic numbers following lanthanum. These elements are called the lanthanides. The lanthanides are silvery metals that tarnish easily. They are relatively soft metals, with high melting and boiling points. The lanthanides react to form many different compounds. These elements are used in lamps, magnets, lasers, and to improve the properties of other metals.Their atomic numbers follow actinium. All of the actinides are radioactive, with positively charged ions. They are reactive metals that form compounds with most nonmetals. The actinides are used in medicines and nuclear devices.Why are these groups mixed. The transition from metal to nonmetal is gradual. Even though these elements aren't similar enough to have groups contained within single columns, they share some common properties. You can predict how many electrons are needed to complete an electron shell. The metals in these groups are called basic metals.Some elements have some, but not all of the properties of the metals. These elements are called metalloids.Solid nonmetals are brittle and lack metallic luster. Most nonmetals gain electrons easily. The nonmetals are located on the upper right side of the periodic table, separated from metals by a line that cuts diagonally through the periodic table. The nonmetals can be divided into classes of elements that have similar properties. The halogens and the noble gases are two groups of nonmetals.Examples of halogens are chlorine and iodine. You find these elements in bleaches, disinfectants, and salts. These nonmetals form ions with a -1 charge. The physical properties of the halogens vary. The halogens are highly reactive.Helium and neon are examples of noble gases. These elements are used to make lighted signs, refrigerants, and lasers. The noble gases are not reactive. This is because they have little tendency to gain or lose electrons.Therefore, hydrogen usually is labeled as a nonmetal.Silicon and germanium are examples of metalloids. The boiling points, melting points, and densities of the metalloids vary. The metalloids make good semiconductors. The metalloids are located along the diagonal line between the metals and nonmetals in the periodic table.Atom size, ease of removing electrons, and ability to form bonds can be predicted as you move across and down the table.What are some other ways you could list and organize the elements? Name an example of each type of element. Retrieved from Trends in the Periodic Table. Preparing for Professional and Graduate Programs Course Descriptions Online Chemistry Textbooks Chemistry Corner Preparing for Professional and Graduate Programs Course Descriptions Online Chemistry Textbooks Chemistry Corner This is a question that has interested man since the age of the Greek philosophers. Like the ancient Greeks we can perform a simple thought experiment that raises a very important question for modern chemistry: suppose you were given a piece of aluminum foil and asked to cut the foil in half over and over. How long could you continue cutting, assuming that you had no limitations based on your own abilities. Is there a limit on how small matter can be broken up into, or could you infinitely divide matter into smaller and smaller pieces. This argument dates as far back as the Greek philosophers. Most, like Aristotle, argued that matter could be divided infinitely. However, one brilliant philosopher, Democritus, argued that there is a limit. He proposed that the smallest piece that any element (like aluminum) can be divided into and still be recognized as that element is an Atom, a word derived from the Greek word atomos, meaning “indivisible”. It is for this reason that Democritus’ ideas on atoms were dismissed until 1808, when John Dalton, an English scientist, proposed four fundamental assumptions based upon observations that we call Dalton’s Atomic Theory. During a chemical reaction, atoms are rearranged, but they do not break apart, nor are they created or destroyed There are about 90 naturally occurring elements known on Earth. Using technology, scientists have been able to create nearly 30 additional elements that are not readily found in nature. Today, chemistry recognizes a total of 118 elements which are all represented on a standard chart of the elements, called the Periodic Table of Elements. Each element is represented by a one or two letter code, where the first letter is always capitalized and, if a second letter is present, it is written in lowercase. For example, the symbol for Hydrogen is H, and the symbol for carbon is C. Some of the elements have seemingly strange letter codes, such as sodium which is Na. These letter codes are derived from latin terminology. For example, the symbol for sodium (Na) is derived from the latin word, natrium, which means sodium carbonate. Elements in the periodic table can be broken up into different general classes based upon similarities in their properties. Going from left to right across the periodic table, the elements can be broken up into metals, metalloids, and nonmetals. Most metals are ductile (can be drawn out into thin wires), malleable (can be hammered into thin sheets), and good conductors of both heat as well as electricity. All metals are solids at room temperature except for mercury. In chemical reactions, metals easily lose electrons to form positive ions. Examples of metals are silver, gold, and zinc. In chemical reactions, they tend to gain electrons to form negative ions. Examples of nonmetals are hydrogen, carbon, and nitrogen. Metalloids can be shiny or dull. Electricity and heat can travel through metalloids, although not as easily as they can through metals. They are also called semimetals. They are typically semi-conductors, which means that they are elements that conduct electricity better than insulators, but not as well as conductors. They are valuable in the computer chip industry. Examples of metalloids are silicon and boron. All of the known chemical elements are arranged in the format of a table. The table has been set up in such a way that the characteristics of each different element can be predicted by their position on the table. (A) On this rendition of the periodic table, you can see that the pink elements on the lefthand side of the table are the metals, while the blue elements on the right are the non-metals (Hydrogen is the only exception to this rule and will be explained in the subsequent sections). The metalloids (also termed semi-metals) occur in a stairstep pattern between the metals and nonmetals and are represented in this diagram by the green elements. (B) Shows the positions of the metals, nonmetals and metalloids on the periodic table. During this chapter, you will learn more about these unique characteristics, called periodic trends. In the universe as a whole, the most common element is hydrogen (about 90), followed by helium (most of the remaining 10). All other elements are present in relatively minuscule amounts, as far as we can detect. On the planet Earth, however, the situation is rather different. Oxygen makes up 46.1 of the mass of Earth’s crust (the relatively thin layer of rock forming Earth’s surface), mostly in combination with other elements, while silicon makes up 28.5. Hydrogen, the most abundant element in the universe, makes up only 0.14 of Earth’s crust. Table 2.1 lists the relative abundances of elements on Earth as a whole and in Earth’s crust. Table 2.2 lists the relative abundances of elements in the human body. If you compare Table 2.1 and 2.2, you will find disparities between the percentage of each element in the human body and on Earth. Oxygen has the highest percentage in both cases, but carbon, the element with the second highest percentage in the body, is relatively rare on Earth and does not even appear as a separate entry in Table 2.1; carbon is part of the 0.174 representing “other” elements. How does the human body concentrate so many apparently rare elements? We obtain oxygen from the air we breathe and the water we drink. We also obtain hydrogen from water. On the other hand, although carbon is present in the atmosphere as carbon dioxide, and about 80 of the atmosphere is nitrogen, we obtain those two elements from the food we eat, not the air we breathe. For example, chlorine, bromine, and iodine react with other elements (such as sodium) to make similar compounds. Likewise, lithium, sodium, and potassium react with other elements (such as oxygen) to make similar compounds. Why is this so? Later that decade, Dmitri Mendeleev, a Russian chemist, organized all the known elements according to similar properties. He left gaps in his table for what he thought were undiscovered elements, and he made some bold predictions regarding the properties of those undiscovered elements. Later, when elements were discovered whose properties closely matched Mendeleev’s predictions, his version of the table gained favor in the scientific community. Because certain properties of the elements repeat on a regular basis throughout the table (that is, they are periodic), it became known as the periodic table. A group, or family of elements, is a vertical column of the periodic table. Elements are placed into families due to their similar properties, characteristics, and reactivities. For example, all of the elements in group 1 (except for hydrogen, which has unique properties) are very reactive and form compounds in the same ratios and with similar properties as other 1 elements. Due to the similarities in their chemical properties, Mendeleev put these elements into the same group and they came to be known as the alkali metals. The alkali metals include: lithium, sodium, potassium, rubidium, cesium, and francium. Alkali metals are among the most reactive metals. This is due in part to their larger atomic radii and low ionization energies, that will be discussed in more details in section 2.8 below. They get their name from ancient Arabic (al qali) because “scientists” of the time found that the ashes of the vegetation they were burning contained a large amount of sodium and potassium. In Arabic, al qali means ashes. Although most metals tend to be very hard, alkali metals have a soft texture, are silvery in color and can be easily cut. They also have low boiling and melting points and are less dense than most elements. Figure 2.4 shows some of the most common families on the periodic table. Group 2 is called the alkaline earth metals. Once again these elements have similar properties to each other.Although many characteristics are common throughout the group, the heavier metals such as Ca, Sr, Ba, and Ra are almost as reactive as the Group 1 alkali metals. They get their name because early “scientists” found that all of the alkaline earth metals were found in the earth’s crust. Transition elements differ from the main group elements (group A elements) in that they tend to be hard and have high densities. They have high melting points and boiling points and can show various oxidation states when forming chemical bonds (this will be discussed further in chapter 3). They often form colored compounds that are highly stable and they can serve as good catalysts. A catalyst is an agent that helps to speed up a chemical reaction without itself being changed in the process. This group contains very reactive nonmetals. The halogens are an interesting group. Halogens are members of Group 17, which is also referred to as 7A. It is the only group in the Periodic Table that contains all of the states of matter at room temperature. Fluorine, F 2 and chlorine, Cl 2 are gases, while Bromine, Br 2, is a liquid and iodine, I 2, and astatine, At 2, are both solids. Another interesting feature about Group 17 is that it houses four (4) of the seven (7) diatomic elements. Diatomic elements only exist in nature as a pair of atoms of the same element that are bonded together. The seven diatomic elements are H 2, N 2, O 2, F 2, Cl 2, Br 2, and I 2. Notice that the latter four are Group 17 elements. The word halogen comes from the Greek meaning salt forming. French chemists discovered that the majority of halogen ions will form salts when combined with metals. The two most significant properties of noble gases is that they are extremely unreactive, rarely forming compounds, and that they all exist as gases at room temperature. We will learn the reason for their unreactivity when we discuss how compounds form in chapters 3 and 4. The first person to isolate a noble gas was Henry Cavendish, who isolated argon in the late 1700s. The noble gases were actually considered inert gases until the 1960s when a compound was formed between xenon and fluorine which changed the way chemists viewed the “inert” gases. In the English language, inert means to be lifeless or motionless; in the chemical world, inert means does not react. Later, the name “ noble gas ” replaced “inert gas” for the name of Group 18. The elements in this group are also gases at room temperature. Individual atoms are extremely small; even the largest atom has an approximate diameter of only 5.4 ? 10 ?10 m. With that size, it takes over 18 million of these atoms, lined up side by side, to equal the width of your little finger (about 1 cm). Several important elements exist as two-atom combinations and are called diatomic molecules. In representing a diatomic molecule, we use the symbol of the element and include the subscript 2 to indicate that two atoms of that element are joined together. The elements that exist as diatomic molecules are hydrogen (H 2 ), oxygen (O 2 ), nitrogen (N 2 ), fluorine (F 2 ), chlorine (Cl 2 ), bromine (Br 2 ), and iodine (I 2 ). Electrons are outside the nucleus and orbit about it because they are attracted to the positive charge in the nucleus. Figures 2.5 and 2.6 depict the structure of an atom. The protons and neutrons of an atom are found clustered at the center of the atom in a structure called the nucleus. The electrons orbit the nucleus of the atom within an electron cloud, or the empty space that surrounds the atom’s nucleus. Note that most of the area of an atom is taken up by the empty space of the electron cloud. Electrons are not in discrete orbits like planets around the sun. Instead there is a probability that an electron may occupy a certain space within the electron cloud (a) The darker the color, the higher the probability that the hydrogen’s one electron will be at that point at any given time. (b) Similarly, the more crowded the dots, the higher the probability that hydrogen’s one electron will be at that point. In both diagrams, the nucleus is in the center of the diagram. As a result, an atom consists largely of empty space. Atomic particles are so small that it is impractical to measure them in grams, instead we use a relative mass scale which makes the numbers much more manageable. You may also see Atomic Mass Units referred to as Daltons (Da) after John Dalton, the English Chemist that first proposed the atomic theory. Carbon-12 has 6 protons and 6 neutrons in its nucleus, meaning that one amu is equal to the average of the masses of a proton and a neutron. The mass of an atom in AMUs is equal to the number of protons and neutrons making up the atom. For example the atomic mass of bromine is roughly 80 amu and its proton number is 35, meaning that bromine has 35 protons and 45 neutrons in its nucleus. These symbols correspond to important values that give you important information about each element (Figure 2.7). The most important value corresponding to characteristics of an element is the proton number, which is also called a tomic number (represented by the mathematical term, Z ). As it turns out, the number of protons that an atom holds in its nucleus is the key determining feature for its chemical properties. In short, an element is defined by the number of protons found in its nucleus. If you refer back to the Periodic Table of Elements shown in figure 2.2, you will see that the periodic table is organized by the number of protons that an element contains. Thus, as you read across each row of the Periodic Table (left to right), each element increases by one proton (or one Atomic Number, Z ). When atoms are in their elemental states, their overall charge is zero and the atoms are neutral. Since protons are positively charged and electrons are negatively charged, this means that when atoms are in their elemental form, the number of protons equals the number of electrons. Therefore, if you know the atomic number of an atom, you also know how many electrons are present in that atom when it is in its elemental form. It is this movement of electrons that facilitates chemical bond formation. Thus, during bond formation the number of electrons around an atom may change, but the atomic number (or number of protons) remains constant and does not change. Each element on the periodic table is represented by the atomic symbol (Cu for Copper, and Te for Tellurium). Sometimes the Atomic Number is written in the upper lefthand corner, and the Atomic Mass in the righthand corner, as shown in this figure. Sometimes, periodic tables will show the atomic number above the element symbol and the atomic mass below the element symbol, as shown in the periodic table in Figure 2.2. The electrons are ignored in the mass calculation because they are so small that they barely add any mass to the atom. Note that the number of neutrons in an atom does not have to equal the number of protons in the atom. At first it was thought that the number of neutrons in a nucleus was also defining characteristic of an element. However, it was found that atoms of the same element can have different numbers of neutrons. Atoms of the same element that have different numbers of neutrons are called isotopes.