General and Analytical Chemistry

Question 1

tendency of an atom to attach to electrons

Answer 1

electronegativity

Question 2

energy required to remove an electron in gaseous state

Answer 2

ionization energy

Question 3

difference between intramolecular and intermolecular forces

Answer 3

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

Question 4

same element and same atomic number but different mass number

Answer 4

isotope

Question 5

isotope with the highest mass number is said to be a

Answer 5

radioactive isotope

Question 6

number of electrons = number of protons

T/F?

Answer 6

True

Question 7

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

Answer 7

alkaline earth metals

Question 8

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

Answer 8

chalcogens/oxygen

Question 9

which group forms salt with metals?

Answer 9

halogen

Question 10

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

Answer 10

transition metals (lanthanides and actinides)

Question 11

shows energy level of atomic orbital

Answer 11

period/series

Question 12

horizontal/column shows

Answer 12

which group

Question 13

vertical/row shows

Answer 13

period/series

Question 14

what are metalloids and state some elements

Answer 14

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

metalloids are:
boron
silicon
germanium
arsenic
antimony
astatine
tellurium

Question 15

metals are characterized as

Answer 15

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

Question 16

nonmetals are characterized as

Answer 16

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

Question 17

how far the outmost electrons from the nucleus

Answer 17

atomic radius/size

Question 18

tendency to remove electrons

Answer 18

metallic character

Question 19

isoelectronic series

Answer 19

same series and same number of electrons

Question 20

radius of isoelectric series can be increased through

Answer 20

increased electrons

Question 21

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

Answer 21

interchange charges

Question 22

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

Answer 22

instead of interchanging, just cancel them out

Question 23

what are oxyanions

Answer 23

oxygen atom + anions

Question 24

how to name mono and poly cation?

Answer 24

mono: as in/parent name

poly cation: -ium

Question 25

name mono/poly anion

Answer 25

-ide

Question 26

transition metals

Answer 26

higher: -ic lower: -ous

Question 27

oxyanions such as bromine, iodine, chlorine

Answer 27

it depends on the number of oxygen such as: 1: hypo-, -ite 2: -ite 3: -ate 4: per-, -ate

Question 28

oxyanions of nitrogen, phosphate, sulfur

Answer 28

higher: -ate lower: -ite ex. nitrate, nitrite

Question 29

other oxyanions

Answer 29

name it with -ate

Question 30

difference between ionic, covalent and metallic compounds

Answer 30

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

Question 31

H+ acts as cation + any anion

Answer 31

inorganic acids

Question 32

how to name inorganic acids

Answer 32

- ite: -ous acid - ide: hydro- -ic acid - ate: -ic acid

Question 33

explain quantum electron theory

Answer 33

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

Question 34

what are quantum number set

Answer 34

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

Question 35

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

Answer 35

principal axis

Question 36

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

Answer 36

orbital increases in size while energy increases

Question 37

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

Answer 37

magnetic

Question 38

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

Answer 38

magnetic spin

Question 39

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

Answer 39

azimuthal

Question 40

what are the different types of radioactive decay?

Answer 40

``` beta alpha positron electron capture gamma ```

Question 41

3 principles applied in filling up orbitals

Answer 41

aufbau, hund's, pauli's exclusion principle

Question 42

explain aufbau, hunds & pauli's

Answer 42

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