chemistry - unit one

Question 1

how many electrons are in a p subshell?

Answer 1

6 electrons

Question 2

how many electrons are in an f subshell?

Answer 2

14 electrons

Question 3

how many electrons are in a g subshell?

Answer 3

18 electrons

Question 4

how many electrons are in a d subshell?

Answer 4

10 electrons

Question 5

how many electrons are in an s subshell?

Answer 5

2 electrons

Question 6

what are isotopes?

Answer 6

atoms of the same element with the same number of protons but different numbers of neutrons

Question 7

what is an ion?

Answer 7

a changed particle when you lose or gain electrons

Question 8

electronegativity

Answer 8

a measure of an atom’s ability to attract shared electrons to itself

Question 9

what are the three types of intermolecular forces?

Answer 9

1) temporary induced dipole-dipole interactions (van der waals forces)
2) permanent dipole-dipole interactions
3) hydrogen bonding

Question 10

what is the weakest type of intermolecular force?

Answer 10

temporary induced dipoe dipole interactions

Question 11

what is the strongest type of intermolecular force?

Answer 11

hydrogen bonding

Question 12

how do induced dipole depend on electrons?

Answer 12

the more electrons = the biigger the force of the induced dipole

Question 13

what 3 factors impact electronegativity?

Answer 13

1) nuclear charge
2) atomic radiius
3) shielding

Question 14

how does nuclear charge affect electronegativity?

Answer 14

the more protons = the stronger the attraction between the nucleus and bonding pairs of electrons

Question 15

how does atomic radius affect electronegativity?

Answer 15

the closer atoms are to the nucleus = the stronger the attraction between the nucleus and bonding pairs of electron

Question 16

what is ionic bonding?

Answer 16

• where an atom of one element loses one or more electrons and donates it to an atom of another element, forming an ion in the process
• there is electrostatic attraction between the oppositely charged ions (metal + non-metal)
• properties include high melting and boiling points, conductors of electricity when molten / insolution, and are able to form crystals

Question 17

how does an atom become positively charged?

Answer 17

when it loses an electron

Question 18

how does an atom become negatively charged?

Answer 18

when it gains an electron

Question 19

electrostatic attraction

Answer 19

the force experienced by oppositely charged particles, holding those particles strongly together

Question 20

ionic bond properties:

Answer 20

• high melting point
• high boiling point
• has a giant ionic lattice

Question 21

what does the strength of the electrostatic force depend on?

Answer 21

• the ionic charge and the ionic radii of the ions
• the more electrons a positive ion has = the more shells it will have = the bigger the ionic radii
• the electrosatic force is stronger when the ionic charge is higjer

Question 22

what are covalend bonds?

Answer 22

• the bond between non-metals with a shared pair of electrons
• covalent bonds have strong electrostatic attraction between nuclei and electrons

Question 23

what are lone pairs?

Answer 23

a non-binding pair of electrons

Question 24

why are metals malleable?

Answer 24

• atoms have layers
• so theyre able to slide over eachother

Question 25

what is the atominc number?

Answer 25

the number of protons in the nucleus of an atom

Question 26

what is the mass number?

Answer 26

the total number of protons and neutrons in an atom

Question 27

electron configuration

Answer 27

the arrangement of electrons in energy levels (shells) around the nucleus

Question 28

how many electrons can the first, second, and third shells hold?

Answer 28

1. 2 2. 8 3. 8

Question 29

define "period" in the periodic table ( -- )

Answer 29

a horizontal row indicating the number of electron shells

Question 30

define "group" in the periodic table ( I )

Answer 30

a vertical column indicating the number of electrons in the outer shell

Question 31

what happens to atomic radius across a period?

Answer 31

it decreases

Question 32

what happens to ionisation energy across a period?

Answer 32

it increases

Question 33

what are the properties of Group 0 (noble gases)?

Answer 33

- unreactive - has a full outer shell - exists as single atoms

Question 34

what are the properties of Group 7 (halogens)?

Answer 34

- they are non-metals - they form diatomic molecules, - slighly reactive at the top of the group

Question 35

what are the properties of Group 1 (alkali metals)?

Answer 35

- very reactive (towards the bottom of thr group) - soft - reacts with water to form hydroxides + hydrogen gas

Question 36

what is the atomic radii?

Answer 36

the distance from the nucleus of an atom to the outermost electron shell

Question 37

describe the trends of the atomic radius of the period table:

Answer 37

Across a period (left → right): - the atomic radius decreases - this is because more protons = stronger attraction pulling electrons closer to the nucleus, even though more electrons are added Down a group (top → bottom): - the atomic radius increases - this is because moree electron shells are added, increasing the distance between the nucleus and outermost electrons

Question 38

compare the properties of SIMPLE- moleculed and GIANT-structured covalent bonds

Answer 38

simple molecules: - low melting/boiling points - do not conduct electricity - usually gases or liquids at room temperature giant structures: - very high melting points - hard - do not conduct electricity (except graphite).

Question 39

what allows metals to conduct electricity?

Answer 39

delocalised electrons that can move freely through the structure

Question 40

what is a giant ionic lattice?

Answer 40

a repeating structure of positive and negative ions held together by strong ionic bonds

Question 41

why do ionic compounds conduct electricity only when molten or dissolved?

Answer 41

ions are free to move and carry charge in those states