chemistry part-2

Question 1

what drives chemistry?

Answer 1

• kind of bonds between atoms in compounds.
• movement of electrons (valence electron at the most outer shell moves around)
• molecule size and shape
• temperature

Question 2

Type of bonds

Answer 2

• Ionic

- covalent

Question 3

how to determined type of bond

Answer 3

by the power of an atom to attract electrons to itself.

Question 4

Covalent bonds

Answer 4

• formed between atoms with similar electronegative.
• share electrons from outer molecular orbit.
• these bonds are formed between non-metal atoms.
• definite shape
• low melting point
• low boiling point
  ex: methane(CH4), hydrochloric acid (HCI)

Question 5

Ionic bond

Answer 5

• formed between atoms with different electronegative.
• one of the atoms will lose the electron to the other atom (in covalent they share)
• transfer of electrons between atoms.
• this results In cation and anion.
• formed between metal and non-metal atoms
• no defined shape.
• high melting point and boiling point
  ex: sodium chloride (NaCl)

Question 6

Cation

Answer 6

positively charged ion (+1)

when they lose electrons.

Question 7

Anion

Answer 7

Negatively charged ion (-1)

when they gain electrons.

Question 8

Electrolytes in body fluid

Answer 8

sodium Na+ 
Chloride  Cl- 
Magnesium Mg2+
Calcium Ca2+
Potassium K+

Question 9

What have full valence electron configuration?

Answer 9

Noble gases means full outer energy level
- last row of periodic table is know as noble gases because it has a full valency election, the outer shell has full electrons.

Question 10

Why electron moves

Answer 10

to becomes as astable as group 18 noble gases

Question 11

Types of molecules

Answer 11

polar and non-polar

Question 12

is single oxygen, O, molecule?

Answer 12

no

Question 13

Types of molecules

Answer 13

polar and non-polar

Question 14

Types of covalent bond

Answer 14

polar and non-polar

Question 15

Polar molecules

Answer 15

• electrons are not equally shared
• one part of molecule is more negative that the other
• so, molecule has negative and positive poles
• hydrophilic (‘water loving’)

Question 16

Non-polar molecules

Answer 16

• electron are equally shared
• there is no poles.
• hydrophobic (water fearing)

Question 17

polar covalent

Answer 17

• atoms with different electronegativities bound together.
• occur between different atom types
• bonding electrons found closer to one atom

Question 18

non-polar covalent

Answer 18

• atoms with similar electronegativities bound together.
• occur between identical atom types
• bonding electrons found halfway.

Question 19

what kind of molecules can be mixed in another

Answer 19

molecules of similar polarity

Question 20

example of polar substances

Answer 20

water, salt, sugar, blood, ammonia, ethanol

Question 21

example of non-polar substances

Answer 21

fat, oil, wax, petrol, butter, soap, bubblegum

Question 22

does oil mix with blood?

Answer 22

no

Question 23

what if you give injection of oil to your patient?

Answer 23

it would form a blood clot because blood is polar as it contains water and oil is non polar.
- only molecule with similar polarities can be mixed.

Question 24

what can trigger different smells in the nose

Answer 24

shape of molecules

Question 25

how does temperature affect chemical

Answer 25

high temperature can change the chemical

Question 26

what is protein denaturation? is it bad?

Answer 26

yes it is

Question 27

lose of shape =

Answer 27

lose of function

Question 28

hydrogen bond

Answer 28

- bond between hydrogen atom and another atom. ex: H2O water - partially electrostatic force of attraction- weaker than covalent or ionic bonds - hydrogen act as a proton donor (positive) - It bonds with another atom with a lone electron pair (negative) - This type of bond can occur in inorganic molecules (water) and in organic molecules e.g. DNA and proteins.

Question 29

is hydrogen bond weaker than covalent or iconic bond

Answer 29

yes

Question 30

element that act as a proton donor

Answer 30

hydrogen

Question 31

what is molecular mass (weight) of compound?

Answer 31

Sum of (relative) atomic masses of the elements in a compound ex: carbon dioxide (compound) carbon (element) - atomic mass 12.1 (x 1- no of atoms) 12 oxygen - atomic mass 16 (x 2) 32 Molecular mass = 12.1 + 32 = 44.01

Question 32

mole

Answer 32

chemical name for specific number of particles in substance. - this could be atoms/ions/molecules - known as Avogadro's number - a really large number - Used as an expression of concentration

Question 33

what is known as Avogadro's number?

Answer 33

mole

Question 34

normal NZ blood glucose?

Answer 34

4-8 millimoles/litre = mol/litre

Question 35

mole equation

Answer 35

``` n = m/M m = mass of material weighted from analytical balance (grams, g) M = molecular mass of material calculated using periodic table. (grams per mol, / g/mol) n= number of moles (unit can be atoms, ions, molecules) ```

Question 36

how many moles are there in 213g of lithium perchlorate (LiClO4)?

Answer 36

``` M = 7 (Li)+ 35.5 (Cl)+ 64 (16x4) (Oxygen) = 106.5g Total   n = 213 g /106.5 g/mol (n=m/M) n= 2 mol ```

Question 37

NZ recommendation: Limit Salt intake per day?

Answer 37

2300 mg per day

Question 38

Excess sodium in blood called?

Answer 38

Hypernatremia

Question 39

What is Normal sodium level?

Answer 39

135–145 mmol/L

Question 40

Symptoms of Hypernatremia

Answer 40

- Thirsty az - vomiting - diarrhoea - fever

Question 41

Concentration definition

Answer 41

amount of stuff(solute) in a bigger amount of stuff (solvent) solute/solvent

Question 42

Volume percentage equation

Answer 42

𝑉𝑜𝑙𝑢𝑚𝑒 𝑝𝑒𝑟𝑐𝑒𝑛𝑡=(𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒)/(𝑣𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛)×100%

Question 43

Mass percentage equation

Answer 43

mass percentage = mass of solute/ mass of solution x100 mass of solute = gram of solute mass of solution = grams of solute + grams of solvent

Question 44

Dose calculation equation

Answer 44

amount to administer = weight x dosage / drug strength

Question 45

therapeutic effect depends on...

Answer 45

concentration and there are many units of concentration.

Question 46

Why do atoms form ions?

Answer 46

Atoms form ions to gain a full valence shell of electrons | when atom loose or gain electrons they form ion.

Question 47

what is electron configuration for a beryllium atom?

Answer 47

2,2

Question 48

Predict the ion formed by beryllium and its electron configuration.

Answer 48

The ion will form when Be loses 2 electrons to become Be2+ with an electron configuration of 2  

Question 49

By transfer of electrons from one atom to another. this is known as________ bonding.

Answer 49

ionic bonding

Question 50

By the share of electrons from one atom to another. this is known as________ bonding.

Answer 50

covalent

Question 51

which statement about non-polar covalent bond is correct? - gain electrons - equally share electrons - lose electrons - unequally share electrons

Answer 51

equally share electrons.

Question 52

Molecules

Answer 52

are atoms that are chemically bonded together and are an electronically neutral group

Question 53

elements react in order to achieve the ________. by doing this they achieve the_______.

Answer 53

full outer energy level. | electronic structure of the noble gases (full outer energy level).

Question 54

When metal reacts with non-metal this is a ____ bonding

Answer 54

ionic