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| ______ proposed that the properties of the elements vary in a periodic manner with the atomic weight of the elements. |
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| Mendeleev grouped elements with similar properties in __rows __columns __groups of eight |
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| In 1914 _____ found that the frequency of vibration of the X-rays emitted by each element when bombarded with cathode rays bore a simple relationship to the atomic numbers |
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| Complete the following: The periodic law specifies... |
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Definition
| "... the chemical properties of the elements are periodic functions of their atomic numbers." |
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| What determines the "energy level" of an electron? |
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Definition
| The distance of the electron from the proton-containing nucleus. |
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| T/F~ The MORE energetic electrons orbit closest to the nucleus. |
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| Who developed the "planetary model" of the atom? |
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| T/F~ SEVEN is the maximal number of electron layers that any atom can contain. |
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| T/F~ Each of the energy levels has a limit on the number of electrons it can hold. |
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| How many electrons can the third energy level hold? |
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| What equation specifies the maximum number of electrons an energy level can hold? |
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| What is the "octet rule"? |
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Definition
| "The maximum number of electrons in the outermost energy level is 8" |
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| What is the "electron configuration?" |
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Definition
| "The number and position of electrons in the energy levels of an atom." |
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| What is the electron configuration of the atom with an atomic number equal to 8? |
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| What is the electron configuration of the atom with an atomic number equal to 16? |
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Definition
| level 1 = 2, level 2 = 8, level 3 = 6 |
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| What is the electron configuration of the atom with an atomic number equal to 20? |
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Definition
| level 1 = 2, level 2 = 8, level 3 = 8, level 4 = 2 |
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Term
| The electrons in the outermost energy level are called... |
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Term
| What about the valence electrons is so important to the field of chemistry? |
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Definition
| The ability of the atom to gain or lose the valence electrons is what determines it's chemical properties. Most chemical reactions involve the valence electrons; electrons in the inner layers are not important in normal circumstances. |
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Term
| Elements in the periodic table are arranged in what two ways? |
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Definition
| Horizontally in rows in the order of increasing atomic number; vertically in columns according to their chemical properties. |
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| T/F~ All elements in vertical columns have same number of valence electrons. |
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| T/F~ Rows in the periodic table are called families or groups. |
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| The alkali metals are located in what group number? |
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| The halogens are located in what group number? |
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| The noble gases are located in what group number? |
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| The alkaline earth metals are located in what group number? |
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Definition
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| T/F~ Chemical properties change across rows, that is as you move from left to right within a period. |
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Definition
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Term
| T/F~ With reference to the electronic configuration a new layer is added for each row or period in the periodic table. |
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| T/F~ The energy lovel of the valence electrons is determined by the period it is in. |
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| T/F~ The shape of the periodic table tells us where all of the electrons are in an atom. |
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Term
| T/F~ The maximal number of electrons in energy level 7 is 98 |
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Term
| Locate aluminum in the periodic table. How many valence electrons is there in a neutral atom of aluminum? |
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| What is the dominant chemical property of the alkali metals group? |
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Definition
| They easily lose theri single valence electron. Thurs they are highly chemically reactive, especially with non mentals. |
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Term
| What are the two most common valences for the "transition elements?" |
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Term
| T/F~ The alkali metals exist in nature as diatomic molecules. |
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Term
| Why are the halogens so extremely reactive chemically? |
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Definition
| They seek an electron to complete their outermost electron level. We say they are highly electronegative. |
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Term
| List the three classes of elements and designate their relative positions in the periodic table. |
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Definition
| metals are on the left side; nonmetals are on the extreme right side; metalloids are in between. |
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| List four properties of metals. |
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Definition
| Conductors of heat and electricity; will lose electrons when reacting with nonmetals; lustrous, malleable, and ductile; have high tensile strength; all are solids at room temperature except for mercury. |
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| Most metals are hard, strong and dense. Provide two examples of metals that are the exceptions to this. |
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Definition
| Sodium (Na) is soft- you can cut it with a knife; Mercury (Hg) is a liquid. Maganese (Mn) is brittle. |
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| T/F~ Metals belong to the families of elements with few electrons (1,2,or3) in the outer energy level. |
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| T/F~ Metals do not hold their valence electrons strongly and give them up easily. |
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