patterns in periodic table – Flashcards

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question
how are elements in the same period arranged?
answer

Each sequential element has one more proton and one electron

 

(as you go from left to right)

question
how are elements in the same group related ?
answer
they have a same valence config & have similar chemical properties
question
grp 1A is called
answer
alkali metals
question
grp 2a is called
answer
alkali earth metals
question
B,Si,Ge, As,Sb,Te,Po are called
answer
metalloids
question
C,N,O,P,S,Se are called
answer
non metals
question
Grp 7A are called?
answer
halogens
question
Grp 8A is called
answer
inert(noble) gases
question
effective nuclear charge def
answer

as the nucleus becomes ↑ positive,

all electrons experience a stronger pull toward the center.

 

"how strong a particular element pulls electrons"

question
Why do cations vs (anions /neutral) have a higher effective nuclear charge?
answer

cations: have more protons than electrons, therefore they are strongly attracted to electrons

(aka they really want to get rid of their positive charge).

 

anions: have more elecs will have a slightly lower effective nuclear charge.

 

neutral: have an equal # of protons and elecs

(have the lowest eff. nuc charge)

question

Who has a larger effective nuclear charge(Zeff):

Na or Mg?

answer

Mg

effective nuclear charge increaes as you go across elements in the same period.

question

Who will have a bigger prinicipal quantum number H or Fr?

whos electrtons will be held less tightly?

answer

Fr ;

as you go  DOWN a grp prinicipal quantum number increases


its  valence e- will be held less tightly to nucleus

 

question
Tell who has a bigger atomic radius K or Mn?
answer

K ;

atomic radii decreases as you go across a period

(recall zeff increases)

question
Ionization energy/potential (IE) def
answer

energy required to remove an electron from a gaseous atom or ion

 

(this requires energy (endothermic))

question

If the effective nuclear charge is high :

describe the location of the valence e-

the ionization energy

the electron affinity

 

answer

high zeff=

valence e- tightly bound to nucleus

HIGH ionization energy

HIGH electron affinity

 

(aka it takes it alot energy to remove these electrons)

question
Why is the second ionization energy always higher than the 1st ionization energy?
answer

Recall an element doesn't want to have a postive charge it wants to gain e- in order to have a full octet,

so it takes alot more energy to remove the 2nd e- ;b/c the element is becoming increasingly positive.

question

Why do grps 1 ; 2 have low electron affinties?

Why do grp 7 have high?

answer

grps 1 ; 2 (alkali metals ;alkali earth metals) need to lose 1 or 2 e- to achieve their octet.

grp 7 (halogens): only need to gain 1 more e- to achieve their octet so they are the greediest.

question

electron affinity def

electronegativity def

answer

1.energy released when atom recieves an electron

*(remember if an element is closer to its octet its energy will be lower hence released , that is a very good thing)

;

2. is a measure of the attractive force that an atom will excert in an electron in a chemical bond, aka its attraction for bonding electrons

question
what is another name for electronegativity?
answer
nuclear positivity
question
True or False: metals have a low density ; high melting points
answer

metals have a high density

high melting point

question

For metals in general give high/low for the following:

zeff;(effective nuclear charge)

electronegativity

atomic radius

ionization energy

answer

;zeff;(effective nuclear charge)

;electronegativity

;atomic radius

;ionization energy

question
;What do the previous characterisitcs allow metals to do?
answer
donate one or more electrons
question
Why are metals good conductors of heat and electricity?
answer
their valence electrons are not bound tightly, they can move freely.
question
  1. For non metals in general give high/low for the following:

    zeff;(effective nuclear charge)

    electronegativity

    electron affinity

    atomic radius

    ionization energy

answer

zeff;(effective nuclear charge)

;electronegativity,electron affinity

;atomic radius

;ionization energy

question

True or False:

Non metals are good conductors of electricity and heat

answer
false
question
Which metals are the most reactive?
answer
alkali and alkali earth
question
alkali metals typically have an oxidation state of?
answer

+1

(they often lose 1 e- to complete their octet)

question
what is the oxidation state of alkaline earth metals
answer

+2

(they like to lose 2 electrons in order to complete their 'octet')

"full outer shell"

question
halogen oxidation state
answer

-1

(prefer to gain 1 e- to complete their octet)

*remember they have 7 electrons

question
true or false: halogens have the highest electronegativities
answer
yes, remember they only need one more e- to complete their octet
question

Noble gases:

Why are they stable?

tell high/low:

ionization energy

electronegativites

answer

their valence shell is complete (8e-)

;

;ionization energy

almost zero ;electronegativites

question

describe the oxidation states of transition metals

give 2 ex

answer

transition metals have many positive oxidation states

Fe: +1 ,+2

Mn: +2,+3,+6,+7

question
transition metals have many positive oxidation states, what does this allow them to do?
answer

form many differnt ionic compounds

ex hydration complexes (water)

highly colored solutes and compounds(enchances the low solubility of some compounds);

question
hemogloblin has what significance regarding this chapter?
answer
hemogloblin features Fe which changes it state in order to carry out its fcn.
question

Why does P have a lower electron affinity than Si?

(this goes agaist the periodic table trend )

answer

P's electronegativity gives a very stable half filled p oribital

vs

Si only needs 1 more electron to fill its p orbital and therefore is very greedy.

question
the grp next to the halogens is called
answer
chalogen
question

which will have a bigger atomic radius?

anion or cation vs a neutral atom

answer

K- (bigger)

than K

b/c its has gained more e-

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