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Chemistry > Unit 7: Periodic Properties/Trends > Flashcards

Unit 7: Periodic Properties/Trends Flashcards

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1
Q

What does isoelectronic mean?

A

ions that posses the same number of electrons, the ion of an element will have the same electron configuration of the closest noble gas

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2
Q

What is a cations size compared to its parent neutral atom?

A

Cations have a smaller radius than their parent neutral atom

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3
Q

What is a anions size compared to its parent neutral atom?

A

anions have a larger radius than their parent neutral atom

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4
Q

What is an isoeletronic series?

A

shows the change in atomic radius due to increasing effective nuclear charge for isoelectronic ions, as teh effective nuclear charge increases the radius decreases (usually placed in decreasing radius order)

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5
Q

What are characteristics for metals?

A
  • silver colored (except gold and copper)
  • high luster (shiny!)
  • malleable-can be shaped and hammered
  • ductile-can be drawn into wires
  • conduct heat very well
  • conduct electricity well
  • exist as solids at room temp (except mercury)
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6
Q

Characteristics of nonmetals

A
  • varied in color (purple iodine, brown bromine, etc)
  • lack luster
  • brittle
  • conduct electricity poorly
  • conduct heat poorly
  • exist in various phases
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7
Q

Characteristics of metalloids

A
  • a mix of metal properties and non-metal properties

* also called semi-conductors -> moderate conductors of electricity

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8
Q

What did Mendeleev do?

A

*insisted on grouping by similar characteristics leaving space for undiscovered elements

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9
Q

What did Moseley do?

A

arranged based on atomic numbers solved some inconsistencies of Mendeleev order

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10
Q

What is ENC? effective nuclear charger

A

how much pull does the nucleus have on electrons

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11
Q

What is electron shielding?

A

The non valence electrons protecting the valence electrons from the nucleus

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12
Q

Fill in

The ____ protons= ___ ENC = ____ attraction of electrons

A
  1. more
  2. greater
  3. greater
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13
Q

What is the equation to find the effective nuclear charge?

A 
Zeff = Z-S
zeff = ENC
Z= number of protons
S= # of core electrons (non valence)
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14
Q

In what trend does ENC increase?

A

from left to right within a period

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15
Q

In what trend does ENC stay the same?

A

from top to bottom

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16
Q

What is electron shielding? and what does it do?

A

the inner electrons (core electrons) act as a barrier between the nucleus and the outer electrons
*limits effect of ENC

17
Q

What trumps or is more powerful that ENC?

A

Electron shielding

18
Q

In what trend does electron shielding stay the same?

A

across a period

19
Q

In what trend does electron shielding increase?

A

down a group

20
Q

In what trend does atomic radius decrease? and why?

A

Across a period

*ENC increases while electron shielding stays the same thus pulls the outer electrons in closer

21
Q

In what trend does radius increase? and why?

A

moving down within a group
*ENC stays constant, but electron shielding increases. The additional energy levels allow the outer electrons to move farther out

22
Q

What do groups mean?

A

Group # = # of electrons (# of electrons in outer shell)

*vertical columns

23
Q

Which group is halogens?
Noble gases?
alkali metals?
alkali earth metals?

A
  • halogens is group 17
  • noble gases is group 18
  • alkali metals is group 1
  • alkali earth metals is group 2
24
Q

Definition of ionization energy

A

the minimum energy required to remove an electron from the ground state of an atom or ion

25
Q

Fill in

The ____ the ionization energy, the ____it is to take off an electron

A
  1. higher

2. harder

26
Q

In what trend does ionization energy increase? and why?

A

from left to right (across any row)

*ENC goes up electron shielding stays constant. therefore, more energy is needed to remove an electron

27
Q

In what trend does ionization energy decrease? and why?

A

from top to bottom (down any column)

*ENC stays the same, electron shielding goes up. Therefore, less energy is needed to remove an e-

28
Q

What is electron affinity?

A

The energy change that occurs when an electron is added to a neutral atom

29
Q

fill in

the ____ the electron affinity, the _____ the attraction of an atom for an electron

A
  1. higher

2. stronger

30
Q

In what trend does electron affinity increase? and why?

A

from left to right (across any row) Electron affinity increases
*ENC increases, shield stays the same stronger attractions for e-

31
Q

In what trend does electron affinity decrease? and why?

A

from top to bottom (down any column) electron affinity decreases
*ENC stays the same, the shielding goes up. Therefore, slightly harder to gain electrons

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