Chemistry chapter 5
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Created by:
cyndydriggs on November 18, 2010
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97 terms
Terms | Definitions |
|---|---|
 Mendeleev. | The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to |
| properties | Mendeleev left spaces in his periodic table and predicted the existence of three elements and their |
| atomic mass | Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing |
| properties | Mendeleev did not always list elements in his periodic table in order of increasing atomic mass because he grouped together elements with similar |
| undiscovered elements | Mendeleev predicted that the spaces in his periodic table represented |
| moseley | the person whose work led to a periodic table based on increasing atomic number was |
| atomic number | Moseley's work led to the realization that elements with similar properties occurred at regular intervals when the elements were arranged in order of increasing |
| permits the properties of an element to be predicted before the element is discovered. | The periodic table |
| atomic number | Evidence gathered since Mendeleev's time indicates that a better arrangement than atomic mass for elements in the periodic table is an arrangement by |
| noble gases | The discovery of what elements added a new column to Mendeleev's periodic table? |
| the actinides | What are the radioactive elements with atomic numbers from 90 to 103 called? |
| the lanthanides | What are the elements with atomic numbers from 58 to 71 called? |
| noble gases | Argon, krypton, and xenon are |
| numbers | The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic |
| number of protons | The periodic law states that the properties of elements are periodic functions of their atomic numbers. What determines the position of each element in the periodic table? |
| the periodic law | The principle that states that the physical and chemical properties of the elements are periodic functions of their atomic numbers is |
| position of the periodic table | The periodic law allows some properties of an element to be predicted based on its |
| the physical and chemicla properties of the elements are hte functions of their atomic numbers. | The periodic law states that |
| properties | Elements in a group or column in the periodic table can be expected to have similar |
| 4 | The atomic number of lithium, the first element in Group 1, is 3. The atomic number of the second element in this group is |
| 18 | How much greater is the atomic number of the fourth element in groups 1, 2 and 18 than the preceding element? |
| 54 | Krypton, atomic number 36, is the fourth element in Group 18. What is the atomic number of xenon, the fifth element in Group 18? |
| 88 | Barium, atomic number 56, is the fifth element in Group 2. What is the atomic number of radium, the next element in Group 2? |
| 18 | For elements in groups 1, 2, and 18, the increase in atomic number for successive elements follows the pattern 8, 8, 18, ?, 32. What number completes the pattern? |
| halogens | Refer to the periodic table. To which group do fluorine and chlorine belong? |
| group. | A horizontal row of blocks in the periodic table is called a(n) |
| period 4 | Refer to the figure above. Potassium and bromine belong to |
| period 3 | The electron configuration of aluminum, atomic number 13, is [Ne] 3s2 3p1. Aluminum is in Period |
| s,p,f,d | Identify the sublevels in a period that contains 32 elements. |
| 2 | How many elements are in a period in which only the s and p sublevels are filled? |
| period 6 | The electron configuration of cesium, atomic number 55, is [Xe] 6s1. In what period is cesium? |
| 2 | Because the first energy level contains only the 1s sublevel, the number of elements in this period is |
| a | In Period 3 there are 8 elements. What sublevel(s) is (are) being filled? |
| a | Period 4 contains 18 elements. How many of these elements have electrons in the d sublevel? |
| electron configuration | the period of an element can be determined from its |
| period 4 | Calcium, atomic number 20, has the electron configuration [Ar] 4s2. In what period is calcium? |
| ... | In the elements Sc, Ti, V, Cr, the s sublevel of the highest occupied energy level |
| metals | Elements to the right side of the periodic table (p-block elements) have properties most associated with |
| a | Neutral atoms with an s2p6 electron configuration in the highest energy level belong to which block of the periodic table? |
| a | Elements in which the d-sublevel is being filled have the properties of |
| a | The group of 14 f block elements in the sixth period is the |
| a | Within the p-block elements, the elements at the top of the table, compared with those at the bottom, |
| a | The electron configurations of the noble gases from neon to radon in the periodic table make these elements part of the |
| a | Hydrogen is placed separately from other elements in the periodic table because it |
| a | To which block do the actinide elements belong? |
| a | The elements whose electron configurations end with s2 p5 in the highest occupied energy level belong to Group |
| a | For groups 13 through 18, the total number of electrons in the highest occupied level equals the group number |
| a | Strontium's highest occupied energy level is 5s2. To what group does strontium belong? |
| a | If n stands for the highest occupied energy level, the outer configuration for all Group 1 elements is |
| a | Titanium, atomic number 22, has the configuration [Ar] 3d2 4s2. To what group does titanium belong? |
| a | Nitrogen's electron configuration is 1s2 2s2 2p3. To what group does nitrogen belong? |
| a | The electron configuration of an element is [Kr] 4d6 5s1. To what group does this element belong? |
| a | Bromine, atomic number 35, belongs to Group 17. How many electrons does bromine have in its outermost energy level? |
| a | Magnesium, atomic number 12, has the electron configuration [Ne] 3s2. To what group does magnesium belong? |
| a | In nature, the alkali metals occur as |
| a | The elements in Group 1 are also known as the |
| a | Which block in the periodic table contains the alkali metals? |
| a | The most reactive group of the nonmetals is the |
| a | The group of soft, silvery, reactive metals, all of which have one electron in an s orbital, is known as the |
| a | The first member of the noble gas family, whose highest energy level consists of an octet of electrons, is |
| a | The most characteristic property of the noble gases is that they |
| a | Compared to the alkali metals, the alkaline-earth metals |
| a | When determining the size of an atom by measuring the distance between bonded, identical, adjacent nuclei, the radius of an atom is |
| a | When an electron is added to a neutral atom, a certain amount of energy is |
| a | Which represents a neutral atom acquiring an electron in a process where energy is released? |
| a | The energy required to remove an electron from an atom is the atom's |
| a | A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called |
| a | One-half the distance between the nuclei of identical atoms that are bonded together is called the |
| a | What is removed when the ionization energy is supplied to an atom of an element? |
| a | When an electron is acquired by a neutral atom, the energy change is called |
| a | The element that has the greatest electronegativity is |
| a | A positive ion is known as a(n) |
| a | A negative ion is known as a(n) |
| a | In a row in the periodic table, as the atomic number increases, the atomic radius generally |
| a | Within a group of elements, as the atomic number increases, the atomic radius |
| a | In the alkaline-earth group, atoms with the smallest radii |
| a | As the atomic number of the metals of Group 1 increases, the ionic radius |
| a | Across a period in the periodic table, atomic radii |
| a | The ionization energies for removing successive electrons from sodium are 496 kJ/mol, 4562 kJ/mol, 6912 kJ/mol, and 9544 kJ/mol. The great jump in ionization energy after the first electron is removed indicates that |
| a | Which is the best reason that the atomic radius generally increases with atomic number in each group of elements? |
| a | The ionization energies required to remove successive electrons from one mole of calcium atoms are 590 kJ/mol, 1145 kJ/mol, 4912 kJ/mol, and 6474 kJ/mol. The most common ion of calcium is probably |
| a | For each successive electron removed from an atom, the ionization energy |
| a | As you move down Group 14 in the periodic table from carbon through lead, atomic radii |
| a | As you move left to right in Period 4 from gallium through bromine, atomic radii |
| a | Hoe does the energy required to remove an electron from an atom changer as you move left to right in Period 4 from potassium through iron? |
| a | The force of attraction by Group 1 metals for their valence electrons is |
| a | The electrons available to be lost, gained, or shared when atoms form compounds are called |
| a | Valence electrons are those s and p electrons |
| a | The number of valence electrons in Group 1 elements is |
| a | In Group 2 elements, the valence electrons are in sublevel |
| a | The number of valence electrons in Group 17 elements is |
| a | For groups 13 through 18, the number of valence electrons is equal to the group number |
| a | In groups 13 through 18, valence electrons may be in sublevels |
| a | Across a period, ionization energies of d-block elements generally |
| a | the first electrons to be removed when d-block elements form ions are the |
| a | Which groups in the main group have lower electronegativity than d-block elements? |
| a | Among the d-block elements, as atomic radii decrease, electronegativity values |
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