From Atoms To Molecules

Question 1

Atomic number is the number of…

Answer 1

Protons

Question 2

Mass number is the number of…

Answer 2

Protons and neutrons

Question 3

Isotopes are…

Answer 3

The same number of protons but different number of neutrons.

Question 4

Cations have more…

Answer 4

Protons than electrons

Question 5

Anions have more…

Answer 5

Electrons than protons

Question 6

Elements are…

Answer 6

Atoms of one type

Question 7

Compounds are…

Answer 7

Atoms of two or more different elements join

Question 8

Molecules are…

Answer 8

Atoms that are stuck together

Question 9

Mole is…

Answer 9

Avogadro’s number
6.022x10*23

Question 10

Molarity is…

Answer 10

The number of moles of solute per litre of solution

Question 11

Relative mass is…

Answer 11

The weighted average of all isotopes

Question 12

Molecular weight is…

Answer 12

The mass of a molecule of a substance.

Question 13

Molar mass is…

Answer 13

The mass of one mole of substance

Question 14

What happens when we go across the periodic table?

Answer 14

Atomic size decreases
Number of valence electrons increases
Electronegativity increases
Oxidising nature increases

Question 15

What happens when we go down the group on the periodic table?

Answer 15

Atomic size increases
Number of valence electrons remains the same
Electronegativity decreases
Oxidising nature decreases

Question 16

What is the definition of organic chemistry?

Answer 16

The chemistry of carbon compounds.

Question 17

What are atomic orbitals?

Answer 17

Electrons are grouped into different shells at different distances from the nucleus.

Question 18

What is the principle quantum number

Answer 18

n
Is the number of shells

Question 19

How many electrons can each shell contain?

Answer 19

2n*2

Question 20

What are the energy levels of the shells?

Answer 20

Further from the nucleus has a higher energy level.
As it can hold more electrons.

Question 21

How many and what sub shells are there?

Answer 21

4 subshells (s,p,d,f)

Question 22

What shape is the s orbital?

Answer 22

Spherical

Question 23

What shape is the p orbital?

Answer 23

Two slim spheres on top of each other.

Question 24

What shape is the d orbital?

Answer 24

4 long tear drop shapes attached at their tails, equally separated.

Question 25

What shape is the f orbital?

Answer 25

8 tear drop shapes attached at their tails separated equally (360)

Question 26

How many orbitals does the s subshell contain?

Answer 26

1

Question 27

How many orbitals does the p subshell contain?

Answer 27

3

Question 28

How many orbitals does the d subshell contain?

Answer 28

5

Question 29

How many orbitals does the f subshell contain?

Answer 29

7

Question 30

The definition of electronic configuration of atoms is…

Answer 30

The number of electrons that an atom possesses, and the orbitals in which those electrons are placed in.

Question 31

What are the valance electrons?

Answer 31

Electrons on the outer most shells.

Question 32

The definition of valence is…

Answer 32

The number of electrons an atom must lose or gain to attain the nearest noble gas.

Question 33

What is the Aufbau Principle of ground-state electronic configuration?

Answer 33

Orbitals and shells fill in order of increasing energy.

Question 34

What is the Pauli Exclusion Principle of ground-state electronic configuration?

Answer 34

Each atomic orbital can hold a maximum of 2 electrons.

Question 35

What is the Hunds rule for ground-state electronic configuration?

Answer 35

When there are 2 or more orbitals of the same energy, electrons go in different directions.

Question 36

What is the octet rule?

Answer 36

Atoms transfer or share electrons to attain a filled shell of electrons (noble gases).

Question 37

What is ionic bonding?

Answer 37

Transferring electrons from one atom to another. Ions have opposite charges, and they attract each other to form an ionic bond.

Question 38

Covalent bonding is…

Answer 38

Electrons are shared rather than transferred.

Question 39

Non-polar covalent bonds is when…

Answer 39

Electrons are shared equally.

Question 40

Polar covalent bonds are…

Answer 40

Unequally shared pair of bonding electrons.

Question 41

What is the definition of electronegativity?

Answer 41

Power of an atom in a molecule to attract electrons to itself.

Question 42

What is the definition of bond polarity?

Answer 42

The amount of partial charge multiplied by the bond length.

Question 43

The 3 different types of intermolecular forces are…

Answer 43

1) dipole-dipole interactions 2) van der walls forces 3) hydrogen bonding

Question 44

What is a dipole-dipole interaction?

Answer 44

Interactions between the positive end of one dipole and the negative end of another dipole.

Question 45

What are van der walls forces?

Answer 45

Relatively weak forces of attraction that exist between non polar molecules.

Question 46

What is hydrogen bonding?

Answer 46

Attractive force between the H attached to an electronegative atom of one molecule and an electronegative atom of the same or different molecule.

Question 47

sp3 hybridisation is…

Answer 47

C forms 4 single bonds

Question 48

sp2 hybridisation is…

Answer 48

C forms a double bond

Question 49

sp hybridisation is…

Answer 49

C forms a triple bond or accumulate double bond.