CHAPTERS 2.1-2.5

Question 1

what is it called when negative particles attract to positive particles?

Answer 1

electrostatic attraction

Question 2

what is an isotope?

Answer 2

atoms that have the same number of protons (atomic number) but different number of neutrons (different mass)

Question 3

what is an ion?

Answer 3

atoms that have lost or gained one or more electrons

Question 4

what is the bohr model?

Answer 4

The Bohr model is a simplified representation of atomic structure proposed by Niels Bohr. It suggests that electrons orbit the nucleus in specific energy levels, and they transition between levels by absorbing or emitting energy

Question 5

what does heating an element do to an electron?

Answer 5

heating an element can cause an electron to absorb energy and jump to a higher energy state

Question 6

what is the electronic configuration of elements in shells of elements?

Answer 6

first shell: 2
second shell: 8
third shell: 8 (can hold 18 but once it contains 8, the next 2 electrons go into the fourth shell)
fourth shell: 2

Question 7

what is the difference between the bohr model and the schrödinger model?

Answer 7

The Bohr model treats electrons as particles in fixed orbits, while the Schrödinger model describes electrons having wave-like properties with probability distributions. The Schrödinger model provides a more comprehensive and accurate understanding of atomic behavior.

Question 8

what is the order of electronic subshell configuration?

Answer 8

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14

Question 9

what is a condensed electron configuration?

Answer 9

configuration of the nearest noble gas in [ ] followed by the remainder, eg. the condensed electron configuration for Fe = [Ar] 3d6 4s2

Question 10

what is the rule for filling electronic subshells?

Answer 10

4s is filled and emptied before 3d and 5s is filled before 4d.

Question 11

what are the exception elements to this rule?

Answer 11

copper and chromium.
Cr: [Ar] 3d4 4s2 ❌
[Ar] 3d5 4s1 ✅
Cu: [Ar] 3d9 4s2 ❌
[Ar] 3d10 4s1 ✅

Question 12

what are critical elements and what are examples of them?

Answer 12

critical elements are considered vital for the worlds economy but are in short supply.
eg. platinum, iridium, helium, palladium, phosphorus

Question 13

what happens to the atomic radii of an element on the period table?

Answer 13

across a period: decreases
(core charge and number of protons increase but shielding remains the same)

down a group: increases
(shells being added)

Question 14

what happens to the electronegativity (attraction of atoms for electrons) of an element on the period table?

Answer 14

across a period: increase
(atom radius decreases and core charge increases. there is a stronger pull of nucleus for valence electrons)

down a group: decreases
(atomic radius increases and there is more shielding/less attraction for electrons)

Question 15

what happens to the first ionisation energy of an element on the period table?

Answer 15

across a period: increase
(atomic radius decreases and it take more energy to remove electrons)

down a group: decrease
(atomic radius increases and valence electrons move further away from the nucleus)

Question 16

what happens to the metallic character of an element on the period table?

Answer 16

across a period: decreases
(less likely to lose electrons as atomic radius/electronegativity decreases)

down a group: increases
(ability to lose electrons and atomic radius increases as electronegativity decreases)

Question 17

what happens to the reactivity of metals on the period table?

Answer 17

across a period: decreases
(atomic radius decreases and valence electrons are held more strongly)

down a group: increases
(atomic radius increases and valence electrons are not held strongly)

Question 18

what happens to the reactivity of non metals on the period table?

Answer 18

across a period: increases
(electronegativity increases)

down a group: decreases
(electronegativity decreases)

Question 19

what is the effective nuclear charge of an atom?

Answer 19

the effective nuclear charge of an atom is a measure of the attractive force felt by the valence shell electrons towards the nucleus

Question 20

what is electronegativity?

Answer 20

electronegativity is the ability of an atom to attract electrons towards itself when forming a chemical bond