1. atomic structure

Question 1

Define atom

Accepted Answer

the smallest component of an element having the chemical properties of that element

Question 2

protons and neutrons (1 word)

Accepted Answer

nucleons

Question 3

relative mass of subatomic particles (1)

Accepted Answer

Proton: 1 Neutron: 1 Electron: 1/1836

Question 4

a . X z

Accepted Answer

A= mass number X= element symbol Z= atomic number

Question 5

proton number/atomic number

Accepted Answer

number of protons in the nucleus of each atom of an element

Question 6

nucleon number/mass number

Accepted Answer

number of neutrons and protons in the nucleus of each atom of an element

Question 7

isotope

Accepted Answer

an atom of an element with the same number of protons but different number of neutrons

Question 8

how are isotopes similar and different from each other ? (2,2)

Accepted Answer

they have the same electronic configuration and chemical properties, but different relative isotopic masses and physical properties

Question 9

anion

Accepted Answer

a negatively charged atom/molecule with more electrons than protons

Question 10

cation

Accepted Answer

a positively charged ion that has fewer electrons than protons

Question 11

in an electric field: how would a proton, neutron and electron behave?

Accepted Answer

proton: deflected to the negative plate
neutron: goes straight through the field
electron: deflected to the positive plate

note that electrons will be deflected at a greater angle than protons because they are lighter

Question 12

angle of deflection formula (of a charged particle)

Accepted Answer

theta = (q/m) k k is a constant, q = charge m = mass theta = angle of deflection

Question 13

relative atomic mass (Ar)

Accepted Answer

(average mass of one atom of an element) / (1/12 x mass of one carbon-12 atom) or: the ratio of the average mass of one atom of an element to the mass of 1/12 of a carbon-12 atom

Question 14

relative isotopic mass

Accepted Answer

(mass of one atom of an isotope of an element) / (1/12 x the mass of one atom of carbon-12) or the ratio of one atom of an isotope of an element to the mass of 1/12 of one atom of a carbon-12 atom

Question 15

isotopic abundance / relative abundance

Accepted Answer

the abundance of each isotope in a mixture

Question 16

what is the principal quantum number and what does it mean

Accepted Answer

it is a set of numbers used to describe the main energy level of an electron
indicates:
relative size of the orbital
relative distance of the electron from the nucleus

bigger n = higher energy level, further distance between electron and nucleus

Question 17

maximum number of electrons in a quantum shell

Accepted Answer

2n^2

Question 18

atomic orbital

Accepted Answer

region of space where there is >90% probability of finding an electron

Question 19

electrons in an orbital (2)

Accepted Answer

max 2, in opposite spins

Question 20

shape of s and p orbitals

Accepted Answer

s: spherical p: dumbbell

Question 21

aufbau (building up) principle

Accepted Answer

electrons in their ground states occupy orbitals in order of energy levels. the orbital with the lowest energy will be filled first

Question 22

hund's rule of multiplicity

Accepted Answer

when filling subshells with more than one orbital, each orbital must be singly occupied before electrons are paired

Question 23

pauli exclusion principle

Accepted Answer

an orbital can hold a maximum of 2 electrons and they must have opposite spins

Question 24

valence electron configuration for s-block and p-block

Accepted Answer

period is the quantum number group: 1. ns1 2. ns2 13. ns2np1 14. ns2np2 15. ns2np3 16. ns2np4 17. ns2np5 18. ns2np6

Question 25

transition metal

Accepted Answer

a d-block element that forms one or more stable ions with a partially filled d-subshell

Question 26

d-block elements that are not transition metals and why:

Accepted Answer

Zinc and scandium Zn only forms Zn2+ (3d10) Sc only forms Sc3+ (3d0)

Question 27

ground state

Accepted Answer

all electrons are at their lowest possible energy levels

Question 28

ionic and atomic radii factors (2)

Accepted Answer

1. number of quantum shells 2. effective nuclear charge

Question 29

effective nuclear charge

Accepted Answer

the net nuclear charge experienced by an outer electron

Question 30

nuclear charge factor

Accepted Answer

number of protons

Question 31

shielding effect

Accepted Answer

presence of inner shell electrons reduces electrostatic attraction between the outermost electrons and the nucleus

Question 32

atomic radius trend down group

Accepted Answer

increases:
as number of quantum shells increase, electrons are further away from the nucleus and radius increases

both nuclear charge and shielding effect increases down the group and hence effective nuclear charge differs little down the group

Question 33

atomic radius trend across period

Accepted Answer

decreases across period

nuclear charge increases due to increase in number of protons in nucleus

shielding effect remains constant

effective nuclear charge increases

stronger electrostatic forces of attraction, atomic radius decreases

from Na to Cl -> decrease
from Cl to Ar -> massive increase
because for other elements, the atomic radii refers to the covalent radii, but for noble gases it's the van the waal's radius

1. atomic structure

All cards