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chemistry > General and Analytical Chemistry > Flashcards

General and Analytical Chemistry Flashcards

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1
Q

tendency of an atom to attach to electrons

A

electronegativity

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2
Q

energy required to remove an electron in gaseous state

A

ionization energy

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3
Q

difference between intramolecular and intermolecular forces

A

intramolecular is the force between atoms while intermolecular force is between molecules

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4
Q

same element and same atomic number but different mass number

A

isotope

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5
Q

isotope with the highest mass number is said to be a

A

radioactive isotope

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6
Q

number of electrons = number of protons

T/F?

A

True

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7
Q

which group/family in the periodic table is hard and easily oxidized?

A

alkaline earth metals

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8
Q

which group from the periodic table forms soft minerals with metals?

A

chalcogens/oxygen

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9
Q

which group forms salt with metals?

A

halogen

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10
Q

which group B is considered hard, lustrous, shiny, increased density, mp and oxidation states?

A

transition metals (lanthanides and actinides)

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11
Q

shows energy level of atomic orbital

A

period/series

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12
Q

horizontal/column shows

A

which group

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13
Q

vertical/row shows

A

period/series

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14
Q

what are metalloids and state some elements

A

these are nonmetals/metals, semiconductors, can be hard to soft

metalloids are:
boron
silicon
germanium
arsenic
antimony
astatine
tellurium
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15
Q

metals are characterized as

A 
good conductors
hard and lustrous
donates electrons
usually solid (only Hg is liquid)
malleable and ductile
low electronegativity & ionization state
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16
Q

nonmetals are characterized as

A

insulators
can be solid, liquid or gas
accepts electrons
high electronegativity & ionization state

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17
Q

how far the outmost electrons from the nucleus

A

atomic radius/size

18
Q

tendency to remove electrons

A

metallic character

19
Q

isoelectronic series

A

same series and same number of electrons

20
Q

radius of isoelectric series can be increased through

A

increased electrons

21
Q

in ionic compounds, what will you do to achieve neutrality between cation and anion?

A

interchange charges

22
Q

if neutrality of ionic compounds are achieved, what will you do?

A

instead of interchanging, just cancel them out

23
Q

what are oxyanions

A

oxygen atom + anions

24
Q

how to name mono and poly cation?

A

mono: as in/parent name

poly cation: -ium

25
Q

name mono/poly anion

A

-ide

26
Q

transition metals

A

higher: -ic
lower: -ous

27
Q

oxyanions such as bromine, iodine, chlorine

A

it depends on the number of oxygen such as:

1: hypo-, -ite
2: -ite
3: -ate
4: per-, -ate

28
Q

oxyanions of nitrogen, phosphate, sulfur

A

higher: -ate
lower: -ite

ex. nitrate, nitrite

29
Q

other oxyanions

A

name it with -ate

30
Q

difference between ionic, covalent and metallic compounds

A

metallic: metal to metal - sea of electrons
covalent: non-metals and non-metals - share electrons (nonpolar - equal sharing, polar - unequal sharing)
ionic: metal to non-metal (cation and anion) - they share electrons through electrostatic attraction

31
Q

H+ acts as cation + any anion

A

inorganic acids

32
Q

how to name inorganic acids

A
  • ite: -ous acid
  • ide: hydro- -ic acid
  • ate: -ic acid
33
Q

explain quantum electron theory

A
  1. electron at ground state energy level
  2. absorbs quanta (definite amount of energy)
  3. electron at higher energy level or excited state
  4. if electron becomes lower state energy level then it emitted light
34
Q

what are quantum number set

A

allowed energy levels of electrons and this usually has 4 sets of qn

35
Q

this qn states the energy level of an electron where it is named as n= 1, 2, 3, 4,…

A

principal axis

36
Q

in principal axis, as n increases what happens to the orbital and energy

A

orbital increases in size while energy increases

37
Q

this qn states the orientation of the orbitals in space (-1, 0 +1)

A

magnetic

38
Q

this qn states the direction spin of the electrons (+/- 1/2)

A

magnetic spin

39
Q

this qn states the shape of the orbital where it is named as 0, 1, 2, 3 (s p d f)

A

azimuthal

40
Q

what are the different types of radioactive decay?

A 
beta
alpha
positron
electron capture
gamma
41
Q

3 principles applied in filling up orbitals

A

aufbau, hund’s, pauli’s exclusion principle

42
Q

explain aufbau, hunds & pauli’s

A

aufbau: start rom lowest to highet energy level
pauli’s: no two electrons must have the same set of quantum numbers
hund’s: finish 1/2 before doing -1/2

chemistry (7 decks)

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