Term
| Where are the most active metals located? |
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Definition
Group 1 Alkali metals
Bottom left on periodic table |
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Term
| Where are the most active nonmetals located? |
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Definition
Group 17, Halogens
Top right on periodic table |
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Term
| As you go from the left to right across a period, the atomic size _____. Why? |
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Definition
| Decreases because an increase in (+) nucleus pulls electrons closer, thus decreasing the atomic size |
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Term
| As you travel down a group, the atomic size _______. Why? |
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Definition
| Increases. Energy levels are added |
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Term
| What is a negative ion called? |
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Definition
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Term
| What is a positive ion called? |
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Definition
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Term
| A negative ion is (bigger/smaller) than its parent (neutral) atom |
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Definition
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Term
| A positive ion is (bigger/smaller) than its parent (neutral) atom |
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Definition
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Term
| As you go from left to right across a period, the first ionization energy generally (increases/decreases), why? |
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Definition
| Increases because the smaller the atom, the harder to remove electrons it is |
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Term
| As you go down a group, the first ionization energy generally (increases/decreases), why? |
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Definition
| Decreases due to the shielding effect (outer electrons in higher energy levels are more easily removed) |
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Term
| What is the shielding effect? |
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Definition
| The idea that outer electrons in higher energy levels are more easily removed because they are further from the nucleus |
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Term
| Where is the highest electronegativity found? |
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Definition
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Term
| Where is the lowest electronegativity found? |
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Definition
| Alkali metals, bottom left |
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Term
| Elements of Group 1 are called what? |
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Definition
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Term
| Elements of Group 2 are called what? |
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Definition
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Term
| Elements of group 3-12 are called what? |
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Definition
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Term
| As you go from left to right across the periodic table, the elements go from (metal/nonmetal) to (metal/nonmetal) |
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Definition
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Term
| Group 17 elements are called what? |
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Definition
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Term
| The most active elements are called what? |
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Definition
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Term
| Group 18 elements are called what? |
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Definition
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Term
| What sublevel is filling across the transition elements |
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Definition
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Term
| Elements within a group have a similar number of what? |
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Definition
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Term
| Elements across a period have the same number of what? |
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Definition
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Term
| A negative ion generally indicates what type of element? |
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Definition
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Term
| As you go down a group, the elements generally become (more/less) metallic |
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Definition
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Term
| The majority of elements in the periodic table are (metals/nonmetals) |
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Definition
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Term
| Elements in the periodic table are arranged according to their ____________. |
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Definition
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Term
| An element with both metallic and nometallic properties is called a ___________. |
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Definition
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Term
| Name 3 contributing scientists who helped to develop the periodic table |
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Definition
Stanislao Canizzaro
Dmitri Mendeleev
Henry Moseley |
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Term
| How did Stanislao Canizzaro contribute to the making of the periodic table? |
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Definition
| He invented a method to determine the atomic mass of elements |
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Term
| How did Dmitri Mendeleev contribute to the making of the periodic table? |
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Definition
| He grouped similar elements, predicted missing elements and their properties, and discovered Scandium, Gallium, and Germanium |
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Term
| How di Henry Moseley contribute to the periodic table? |
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Definition
| He noted positive charge of the nucleus incrased by 1 from one element to the next, discovered the atomic number |
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Term
| Why did Mendeleev leave empty spaces on his periodic table? |
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Definition
| For the placement of still undiscovered elements |
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Term
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Definition
| The physical and chemical properties of the elements are periodic functions of their atomic numbers |
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Term
| Which elements are disignated as the alkali metals? List characteristic properties. |
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Definition
| Group 1- they are soft to cut, silvery, reactive, have 1 valence electron |
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Term
| Which elements are designated as the alkaline earth metals? How do their properties compare to the alkali metals? |
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Definition
| Group 2, they are harder and denser and less reactive than the Alkali metals |
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Term
| What is the name used to refer to the entire set of d-block elements? |
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Definition
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Term
| Why do the properties of the p-block elements differ so greatly? |
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Definition
| Because they consist of metals, nonmetals, and metalloids |
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Term
| Which elements are designated as the halogens? What are some characteristics of halogens? |
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Definition
| Group 17-They have 7 valence electrons, most-reactive nonmetals, and form salt with metals |
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Term
| Which elements are designated as the noble gases? List characteristic properties, too. |
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Definition
| Group 18- Are unreactive (inert gases) that have 8 valence electrons (octet) |
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Term
| Which groups of metals make up the f-block on the periodic table? |
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Definition
| The lanthanides and actinides |
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Term
| Why is the "periodic table" not just called the table of elements |
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Definition
| Because the elements are arranged due to periodic properties |
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Term
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Definition
| A positive ion, usually metals, that lose electrons therefore decreasing in atomic radii compared to the neutral atom |
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Term
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Definition
| A negative ion, usually nonmetals, that gain electrons, therefore increasing in atomic radii |
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Term
| Of K, Ga, and Br, which has the smallest atomic radius? |
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Definition
| Br, as you move left to right atomic radii decreases because nucleus charge increases |
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Term
Which of the following cations is least likely to form?
Sr+2, Al+3, K+2 |
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Definition
| K+2 because it only needs to lose 1 electron to stabilize, it would take a lot of energy for K to lose the second electron |
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Term
| Why do halogens tend to form -1 anions? |
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Definition
| Because halogens stabilize by gaining 1 electron |
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Term
| What is electronegativity? |
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Definition
| The amount of energy needed to attract an electron |
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Term
| What does a low electronegativity pertain to? |
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Definition
| A low attraction for electrons |
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Term
| What is ionization energy? |
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Definition
| The amount of energy needed to remove 1 electron |
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Term
| What does a low ionization energy pertain to? |
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Definition
| Electron is easily removed |
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Term
| What is electron affinity? |
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Definition
| The amount of energy change when electron is acquired |
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Term
| What does high electron affinity pertain to? |
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Definition
| A high release of energy when an electron is added |
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Term
| Where are metalloids found on the periodic table? |
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Definition
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