Merrill Chem. Ch. 10 Word Scramble
|
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Question | Answer |
Elements in the same column have similar... | outer level electron configurations |
Outer level electron configurations change in a regular way from... | one column to the next |
Properties are... | periodic |
What kind of elements have the highest density? | Metals |
What kind of elements have the lowest density? | Nonmetals existing as gases at room tempereature |
As the principle quantum number increases, the size of the electron cloud... | increases |
How does the size of atoms develop as you look down the table? | It increases |
Why does the size of atoms decrease as you move across a period? | One proton is added with each element, which means the electron cloud is pulled in tighter each time |
How does the atomic radii of atoms increase? | Top to bottom and right to left |
The density pattern is... | low-high-low |
In general, when atoms form to unite compounds... | the compound is more stable than the uncombined atoms |
Noble gas configurations are particulartly stable because... | the noble gases have filled outer energy levels |
Chemists discuss the size of ions by referring to their... | ionic radii |
Metallic ions, on the left and in the center of the table, are formed by... | the loss of electrons |
Nonmetallic ions, located on the right side of the table, are formed by... | the gain of electrons and are larger than the atoms from which they are formed |
Metallic ions have an outer level that resembles that of... | the noble gas at the end of the preceding period |
Non metallic ions have an outer level resembling that of... | the noble gas to the right of the same period |
The loss of one electron from the metals in Group 1 will give them the same configuration as... | a noble gas |
What is the oxidation number of Group 1? | 1+ |
What is the oxidaton number of Group 2? | 2+ |
What is the oxidation number of Group 13? | 3+ |
What is the oxidation number of Group 14? | 2+ or 4+ |
What is the oxidation number of Group 15? | 3- |
What is the oxidation number of Group 16? | 2- |
What is the oxidation number of Group 17? | 1- |
What is the oxidation number of Group 18? | 0 |
What is ionization energy? | The energy required to remove an electron from an atom |
What is first ionization energy? | The energy required to remove the loosest electron from an atom |
What is ionization energy mesured in? | Kilojoules per mole (kJ/mol) |
How does the first ionization energy change as atomic number increases with a period? | It increases |
How does the first ionization energy change as atomic number increases with a group? | It decreases |
First ionization energy can help classify elements into... | metals or nonmetals |
What kind of first ionization energy do metals have? | Low FIE |
What kind of first ionization energy do nonmetals have? | High FIE |
As you go down a column of the periodic table, first ionization energy... | decreases |
What are two things that tend to lower first ionization energy? | Increased distane of the outer electrons from the nucleus and the sheilding effect |
What is the sheilding effect? | When inner electrons block the attraction of the nucleus for outer electrons |
The number of electrons in the outermost sublevel is the same for all elements in a particular... | group |
Why does first ionization energy increase as you move across a period? | Because the nuclear charge increases |
What are the four factors that affect ionization energy? | 1. Nuclear Charge- up, up 2. Sheilding Effect- up, down 3. Radius- up, down 4. Sublevel- an electron from a full or half-full sublevel requires additional energy to be removed |
The first ionization removes a __ electron. | *p electron |
The second ionization removes a __ electron from a full __ sublevel. | *s electron, s sublevel |
Are the second and third electrons in different or the same sublevels? | They are in the same |
Why is the third electron's ionization energy greater? | Because the positive nuclear charge remains constant as you remove electrons |
What is electron affinity? | The attraction of an atom for an electron |
The same factors that affect ionization energy also affect... | electron affinity |
As electron affinity increases, a(n) ____ in ionization energy can be expected. | Increase |
Metals have ___ electron affinities. | Low |
Nonmetals have ___ electron affinities. | High |
As you go down a group, the tendency to gain electrons _____. This is because atoms farther down the column are lerger. (The nucleus is farther from the surface, and attracts the outer electrons ___ strongly.) | Decreases, less |
As you move across a period (left to right) what happens to the attraction for electrons? | It increases |
Are positive ions smaller or larger than the atoms from which they are produced? | Smaller |
Are negative ions smaller or larger than the atoms from which they are produced? | Larger |
Metals tend to ____ electrons. This means they have positive oxidation numbers. | Lose |
Nonmetals tend to ____ electrons. This means they have negative oxidation numbers. | Gain |
Created by:
hannahb11
Popular Chemistry sets