Chapter 6 Flashcards

0
Q

What do the colors an element is written in stand for?

A
  • Black: Solid at room temp
  • Red: Gas at room temp
  • Blue: Liquid at room temp
  • Grey: Do not exist in nature
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1
Q

What does the vertical column of numbers on a element on the periodic table stand for?

A

-The number of electrons in each occupied energy level

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2
Q

Noble Gases

A
  • The elements in Group 8A of the periodic table
  • Also called inert gases because rarely take part in chemical reaction
  • The s and p sublevels (if they have a p sublevel) are completely filled with electrons
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3
Q

Representative Elements

A
  • Group 1A to 7A on the periodic table
  • Called this because have a wide range of physical and chemical properties
  • Are either metals, metalloids or nonmetals
  • Most are solids, some are gases, and only one (bromine) is a liquid at room temp.
  • The s and p sublevels of the highest energy level are not filled
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4
Q

Transition Elements

A
  • All the Group B elements (entire D block)
  • Two types: Transition metals and inner transition metals
  • Used to be referred to as “rare earth metals”–> misleading because some transition metals are more abundant than other elements, and some inner transition metals cannot be found in nature
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5
Q

Transition Metals

A
  • Part of Group B on the periodic table
  • Displayed in the main body of the periodic table
  • The highest occupied s sublevel and a nearby d sublevel contain electrons
  • Characterized y the presence of electrons in d orbitals
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6
Q

Inner Transition Metals

A
  • Below the main body of the periodic table
  • The highest occupied s sublevel and a nearby f sublevel generally contains electrons
  • Characterized by the presence of electrons in f orbitals
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7
Q

Alkali metal

A

-Any metal in Group 1A of the periodic table

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8
Q

Alkaline Earth Metal

A
  • Any metal in Group 2A of the periodic table
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9
Q

Halogen

A

-A nonmetal in Group 7 of the periodic table

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10
Q

Periodic tables contain what?

A
  • Each element’s name
  • Symbol
  • Atomic number
  • Atomic mass
  • Number of electrons in each energy level
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11
Q

How can an elements electron configuration be determined?

A

-By its location on the periodic table

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12
Q

Atomic Radius

A
  • One-half of the distance between the nuclei of two atoms of the same element when the atoms are joined
  • Measured in picometers
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13
Q

Ion

A
  • An atom or group of atoms that has a positive or negative charge
  • Form when electrons are transferred between atoms
  • Positive ion: Cation
  • Negative Ion: Anion
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14
Q

Cation Charge

A
  • Positive
  • Written as the number for the charge and a plus sign
  • If the charge is 1, just used a plus sign
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15
Q

Anion Charge

A
  • Negative Charge
  • Usually written as the number of the charge and a negative sign
  • If the charge is 1, just a negative sign is used
16
Q

What type of elements tend to form anions, and what type of elements tend to form cations?

A
  • Nonmetals form anions

- Metals form cations

17
Q

Ionization Energy

A
  • The energy required to remove an electron from an atom
18
Q

First ionization Energy

A

-The energy required to remove the first electron from an atom

19
Q

Who made the periodic table

A
  • Dimitri Mendeleev

- Ordered in increasing atomic mass

20
Q

Cations are always…

A

smaller than the atoms from which they form

-size decreases across period

21
Q

Anions are always…

A

larger than the atoms from which they form

-size decreases across period

22
Q

Ionic Size

A

-The size of an atom after receiving or removing an electron(s)

23
Q

Electronegativity

A
  • The ability of an atom of an element to attract electrons when the atom is in a compound or molecule
  • Lowest .7, highest 4.0
24
Electron Shielding
- The one of the two forces that effect atomic size - how electrons are attracted to the nucleus - the more the valence electrons are blocked from the nucleus by other electrons - This makes atoms larger^^ - Electron Shielding is dominant over Nuclear Charge - constant across period, increases across group
25
Metals
- 80% of periodic table - Good conductors of heat and electricity (best= silver, second best= copper) - Freshly cleaned metal will have a sheen (can reflect light) - All metals are a solid @ room temp. (except mercury) - Metals= ductile (can be turned into wire) - Most metals= malleable ( able to be made into sheets without breaking)
26
Nonmetals
- Most nonmetals are gases @ room temp - few= solids (phosphorus, sulfur) - Nonmetal that is liquid= bromine - Because of many different types of nonmetals, no set characteristics - Hard non-metals (diamond), brittle (break if hit)nonmetals (phosphorus) - Poor conductors of heat & electricity
27
Metalloids
- Has properties similar to metals and nonmetals - Under some conditions, act like metals, in other conditions act like nonmetals - Poor conductor of electricity
28
Core electrons
- The electrons blocking the valence electrons | - Part of the inner energy levels
29
Nuclear Charge
- One of the two forces that effect atomic size - How the nucleus attracts electrons - does not effect valence electrons if other energy levels w/ electrons block them - makes atoms smaller becuz of this^^^ - increases across period and group
30
Direction of group and period
- group: vertical | - period horizontal
31
Trend: Decreases group, increases period
- Ionization energy | - Electronegativity
32
Trend:Increases group, decreases period
- Atomic size | - Ionic size