Flashcards
Chapter 6
Cards in this deck (25)
- 1calculating the atomic radiushalf the distance between 2 identical atoms of the same elements, r=d/2
- 2unit of atomic radius and whypicometer (Pm) because the distance between the atoms are extremely small
- 3what are the trends among the elements for atomic size?- size increases from top to bottom within a group
-size decreases for the left to right across a period - 4(GROUP TREND IN ATOMIC SIZE) give an example of a group trend in atomic sizeThe atomic radius increases within these groups as the atomic number increases. As the atomic number increases, the charge on the nucleus increases, and the number of occupied energy levels increases. the shielding effect is greater than the effect of the increase in nuclear charge, so the atomic size increases.
- 5(PERIOD TRENDS IN ATOMIC SIZE) give an example of a period trend in atomic sizeacross a period, electrons are added to the same energy level. the shielding effect is constant. the increasing nuclear charge pulls the electrons of the highest occupied energy level closer to the nucleus, so the atomic size decreases.
- 6anionan ion with a negative charge
- 7ionization energyenergy required to lose electrons from atom
- 8when is ionization energy measured?when the element is at its gaseous state
- 9what are the trends among the elements for first ionization energy?-energy decrease from top to bottom within a group
-energy increase from left to right across a period - 10(GROUP TRENDS IN IONIZATION ENERGY) is it easier or difficult to remove an electron within a group?going down a group, there is more shielding, there are more energy levels, the electrons are further away from the nucleus, so it easier to remove an electron therefore less energy is used
- 11(PERIOD TRENDS IN IONIZATION ENERGY) is it easier or difficult to remove an electron across a period?across a period, you have more protons inside the nucleus, and more attraction between the nucleus and the electronic cloud, which makes it more difficult to remove an electron, therefore, more energy
- 12what happens to the atomic radii and the ionic radii in a cationthe atomic radii will become greater than the ionic radii
atomic radii > ionic radii - 13what happens to the atomic radii and ionic radii in an anionthe atomic radii will become less than the ionic radii
atomic radii < ionic radii - 14what are the trends among the elements for ionic size?-size generally increases from top to bottom within a group
-size of cation and anion decreases from left to right across a period - 15cations are always __________than the atoms from which they formsmaller
- 16anions are always _________than the atoms from which they formlarger
- 17(GROUP TRENDS IN IONIC SIZE)C
- 18(PERIOD TRENDS IN IONIC SIZE)C
- 19when an atom loses electrons what happens to their attraction between the nucleus METALS TEND TO LOSE ELECTRONSincreases. as a result the electrons are drawn closer to the nucleus
- 20when an atom gains electrons what happens to their attraction between the nucleus NONMETAL TEND TO GAIN ELECTRONSdecreases, as a result the electrons are drawn away from the nucleus
- 21ELECTRONEGATIVITYThe ability of an atom to attract electrons even when the atom is in a compound
- 22what are the trends among the elements for electronegativity?-decrease from top to bottom in a group
-increase from left to right across a period
usually for representative elements - 23what happens to elements with less electronegativityless tendency to attract electrons. when it reacts, it tends to lose electrons and form a cation
- 24what happens to an element with more electronegativitystrong tendency to attract electrons. when it bonds. it attracts the shared electrons or forms an anion
- 25summary and all the trends (group) 1)atomic size will increase 2) ionic size will increase 3) nuclear charge will increase 4) shielding effect will increase 5) first ionization energy decrease 6) electronegativity will decreasesummary and all the trends ( across a period)
1) atomic size will decrease
2) cation and anion will decrease
3) nuclear charge will increase
4) shielding effect is constant
5) first ionization energy will increase
6)electronegativity increase
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- Chemistry Flashcards on Chapter 6, created by Lara abudayeh on 31/12/2020.
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- Lara abudayeh
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