Term
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Definition
| Distance from the outermost stable electron orbital to the atomic nucleus |
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Term
| As you go to the right, or across period, atomic radius _________ due to? |
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Definition
| Decreases because of the effective nuclear charge increases, thus attracting orbiting electrons and lessening the radius |
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Term
| As you go to the down, or down a group, atomic radius _________ due to? |
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Definition
| Increases due to the addition of a new energy level (shell) |
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Term
| Regarding to atomic radius, the number of ______ has a large effect on the atomic radius |
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Definition
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Term
| What is Ionization Energy? |
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Definition
| The minimum amount of energy required to remove one electron from each atom in a mole of atoms in the gaseous state. Pretty hard so don't know really all of it but know the basic. How's studying going? |
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Term
| The first ionization energy is |
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Definition
The energy required to remove the atom's nth electron, after the (n−1) electrons before it have been removed.
OR
The energy required to remove the outermost (highest energy) electron from a neutral atom in its ground state. |
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Term
| Ionization energy _____ as you go across a period because |
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Definition
| Increases because the greater number of protons (higher nuclear charge) attract the orbiting electrons more strongly, thereby increasing the energy required to remove one of the electrons. |
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Term
| Ionization energy _____ as you go down a period because |
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Definition
| Decreases because the valence electrons are farther away from the nucleus and experience a weaker; attraction to the nucleus's positive charge |
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Term
| The ______ the principal quantum number, the _________ the ionization energy for the _______ within that shell. |
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Definition
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Term
| Ionization energy trend exceptions |
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Definition
| Oxygen and Boron. However, only slightly less and MAYBE will not have a huge affect |
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Term
| What is Electron affinity |
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Definition
| The energy gained by an atom when an electron is added to it, or conversely as the energy required to detach an electron from a singly charged anion. |
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Term
| What happens to atoms that gain and e- but become more stable? |
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Definition
| For atoms that become less stable upon gaining an electron, potential energy increases, which implies that the atom gains energy. In such a case, the atom's electron affinity value is positive |
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Term
| Atoms with a more negative electron affinity are considered to have a ______ _______ ______ which means |
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Definition
| Consequently, atoms with a more negative electron affinity value are considered to have a lower electron affinity (they are more receptive to gaining electrons), and vice versa. |
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Term
| The energy value obtained when when an e- is detached will |
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Definition
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Term
| Atoms with a _____ electron affinity are less inclined to give up an e-, so it takes more _______ to remove it |
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Definition
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Term
| The atom with the more _______ energy value has the higher electron affinity. |
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Definition
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Term
| As one goes across a period the electron affinity _________ |
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Definition
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Term
| As one goes up a group, the electron affinity |
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Definition
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Term
| What is electronegativity |
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Definition
| Ability of an atom to attract e- to itself in a covalent bond |
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Term
| As one moves across a period, electronegativity _______ and why |
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Definition
| Increases due to the stronger attraction the atoms obtain as the nuclear charge increases |
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Term
| As one moves down a group, electronegativity _____ due to |
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Definition
| Decreases due to the longer distance between the nucleus and the valence electron shell. Thus decreasing the attraction, making the atom have less of an attraction for electrons or protons. |
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Term
| Which atoms does electronegativity increase from in groups 13. And what is odd about group 14 |
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Definition
In 13, Aluminum to Thallium
In 14, Lead has a higher electronegativity then Tin (Sn) |
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Term
| Metallic property ______ across a period due to |
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Definition
| Decreases due to the increase of valence e- and decrease of atomic radius |
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Term
| Metallic property ______ down a group due to |
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Definition
| Increases due to the increase in number of shells and atomic radius |
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Term
| Non-metallic property ______ across a period due to |
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Definition
| Increases due to the increase of valence e- and decrease of atomic radius |
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Term
| Non-metallic property ______ down a group due to |
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Definition
| Decreases due to the increase in number of shells and atomic radius |
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Term
| Anions, which are ______, are _______ than their respective atoms |
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Definition
| Anions (negative ions) are larger than their respective atoms. |
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Term
| Cations which are ______, are _______ than their respective atoms |
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Definition
| Cations (positive ions) are smaller than their respective atoms. |
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Term
| In nonmetals, the elements in the first period have _______ electron affinities than the elements below them in their respective groups |
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Definition
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Term
| The noble gases have very _____ ionization energies and ___ has the highest |
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Definition
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Term
| Metals have a ______ melting ______ |
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Definition
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Term
| MOST non-metals have _____ melting points |
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Definition
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Term
_____ has the highest boiling point
_____ which is a ___-___ also has a high melting point |
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Definition
Carbon
Boron which is a semi-metal |
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Term
| Metallic character relates to the ability to ______ _______, and nonmetallic character relates to the ability to ______ _______. |
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Definition
Lose electrons
Gain electrons |
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Term
| _____ tend to have a higher density because of their _______ |
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Definition
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Term
| As you go down a table, density ______ minus the transition metals |
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Definition
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Term
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Definition
| Properties intermediate with that of metals and nonmetals, the staircase |
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Term
| _____ and _______ are the most abundant elements in Earth's crust, in seawater, and in biological systems |
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Definition
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Term
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Definition
| Nitrogen, potassium, and phosphorus |
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Term
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Definition
| Crimson red yellow Lilac=blueish |
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Term
| _____ lamps are used for commercial and highway lighting |
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Definition
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Term
| Seven-up originally contained |
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Definition
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Term
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Definition
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Term
Colors when burned:
Calcium
Strontium
Barium |
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Definition
Brick red
Crimson red
Green |
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Term
| Inside of Jupiter and Saturn are made of metallic |
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Definition
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Term
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Definition
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Term
| Group __ are known as halogens |
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Definition
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Term
| What is an isoelectronic series? |
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Definition
| A series of ions with the same number of electrons |
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Term
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Definition
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Term
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Definition
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Term
| Effective nuclear charge normally ______ as you go _____ a group because the electrons get farther and farther away from the ______. |
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Definition
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Term
| Going across the table, Effective nuclear charge _______ because the ______ do not move farther away from the nucleus |
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Definition
| Increases because the electrons |
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Term
| Moving ____ the periodic table does ______ then going _______ to the metallic characteristics |
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Definition
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Term
| Zeff is the same thing as |
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Definition
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Term
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Definition
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Term
Ferromagnetism
_____ magnetes
_____ attraction
_____ times stronger then paramagnetism |
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Definition
Permanent
Delocalized
1,000,000 |
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Term
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Definition
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Term
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Definition
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Term
| As you go to the across a period, density ____ |
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Definition
| Peaks at Ti or THE MIDDLE NOT SURE ASK TOMORROW |
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Term
| As Zeff increases, shielding _____ |
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Definition
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Term
| As Zeff decreases, shielding _____ |
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Definition
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Term
| Sulfur is usually found as a ____ _____ |
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Definition
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Term
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Definition
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Term
Zr and Hf are about the same size due to |
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Definition
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Term
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Definition
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Term
| Which 3 atomic trends are the same, trend-wise? |
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Definition
| Ionization energy, Electronegativity, and Electron affinity |
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Term
Things that differ in properties of metals and nonmetals
1.
2.
3.
4.
5. |
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Definition
Metals- Shiny luster; Nonmetals opposite
Metal- Solids are malleable and ductile Nonmetals opposite
Metals Good conductors of heat and electricity Nonmetals opposite
Metals- Metal oxides are ionic and basic Nonmetals opposite
Metals- Form cations in aqueous solutions Nonmetals- Anions in aqueous |
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