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Biology gr12 > chem gr 11 review > Flashcards

chem gr 11 review Flashcards

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1
Q

How do isotopes of the same element differ from each other?

A

An isotope differs in abundance, atomic mass and neutrons. It has the same protons and atomic number.

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2
Q

What is the purpose of using radioactive tracers in medical imaging?

A

Injected into the body of
patients to detect abnormalities such as cancer

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3
Q

Radioisotopes can cause..

A

Cancer, but can also be used for medical purposes.

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4
Q

Unstable isotopes are called..

A

radioisotopes

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5
Q

What are isotopes?

A

Atoms of the same element with the same atomic
number but different atomic mass are called isotopes.

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6
Q

Electronegativity - elements on the left side vs the right side

A

Elements on the left side of the periodic table have little tendency to accept
electrons, elements on the right side have a high tendency to accept electrons.

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7
Q

Explain how ionic bonds are formed. Provide an example of an ionic bond between two elements.

A

Sodium and chlorine, ionic bonds are formed by cations and anions.

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8
Q

ionic bonding occurs…

A

It occurs between non metals and metals, metals lose electrons to non metals (attractions between ions)

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9
Q

What is half life

A

the time taken for half the sample of a
radioactive isotope to decay into another element

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10
Q

What is covalent bonding

A

sharing e-
between atoms/two non metals to create molecules
with a stable electronic configuration.

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11
Q

Non metals are cations or anions? Accepting electrons or donating?

A

Non metals accept electrons and are anions

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12
Q

Metals are cations or anions? Accepting electrons or donating?

A

cations, they donate

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13
Q

What are valence electrons

A

The electrons in the
outermost shell of
an atom. Determines the
chemical and
physical properties
of an element

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14
Q

Elements that have a _______ in
their electronegativity are most
likely to form _________

A

Large difference, ionic bonds

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15
Q

non-metals that are close together on the
periodic table, and have a small
difference in their Electronegativity are likely to form a

A

covalent bond

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16
Q

Electronegativity increases as….

A

you move to the right across the
periodic table

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17
Q

Electronegativity decreases as..

A

You move down the columns or family

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18
Q

non polar covalent bond is

A

e- in the bond are shared equally
between the atoms

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19
Q

polar covalent bond is

A

e- are NOT shared equally

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20
Q

What is electronegativity

A

The desire of an element
to gain electron(s) and to measure the ability of an atom when attracting electrons.

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21
Q

Polar covalent bond is caused by

A

a difference in electronegativity

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22
Q

For a molecule to be polar, it must
contain:

A

polar bonds, asymmetric axis offering a partial
+ve and a partial –ve end.

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23
Q

Ionic compounds when pure have what type of structure

A

crystal lattice

24
Q

What is inTRAmolecular

A

within molecules (covalent
bonding)

25
Q

What is inTERmolecular

A

The forces of attraction or repulsion between neighboring particles, this determines the physical properties

26
Q

What are the two Van der Waals Forces

A

London Dispersion forces and Dipole-dipole forces

27
Q

Difference between London Dispersion forces and Dipole-dipole forces

A

noanswer

28
Q

Which intermolecular
forces that hold non-polar
molecules together?

A

London dispersion

29
Q

Which is the weakest forces of attraction
between all atoms and
molecules.

A

London dispersion

30
Q

Which intermolecular force can hold polar molecules together?

A

Dipole-dipole

31
Q

Dipole-dipole is stronger or weaker than L.D?

A

Stronger

32
Q

What is the strongest intermolecular force?

A

Hydrogen bonds

33
Q

What is hydrogen bonds?

A

A strong
dipole-dipole force
that forms between a
H of one polar
molecule and a N,
O, or F of another
polar molecule

FON

34
Q

Ions are formed when ..

A

atoms gain or lose. electrons

35
Q

what are the differences in electronegativity for polar, non polar and ionic

A

non.p is 0 to 0.5
polar is 0.5 to 1.7
ionic is 1.7 to 3.3

36
Q

What is an isomer

A

same formula, different structure

37
Q

What is hydrophobic? give examples

A

hates water, not soluble in water ex. nail polish, oil, lotion, most paints

38
Q

What is hydrophilic? Give examples

A

Water loving, is soluble in water. Ex. Milk, sugar, syrup, tea

39
Q

What is a lone pair of electrons

A

one pair of unshared electrons on an atom.

40
Q

What helps to
predict molecular shape.

A

VSPER - Valence shell electron pair
repulsion

41
Q

The types of atoms determines..

A

The
types of bonds

42
Q

The arrangement in molecular polarity of bonds will
determine …

A

shape and polarity
of the molecule

43
Q

What will Shape and polarity determine?

A

The type of intermolecular forces between molecules

44
Q

What is molecular shape

A

Non bonding pairs of e- take up more space. They compress the bond angles
of bonding pairs

45
Q

What is complete combustion?

A

Water + carbon dioxide

46
Q

What is incomplete combustion

A

No excess oxygen (air supply is limited) leads to carbon monoxide

47
Q

What are the two chemical bonds

A

covalent and ionic

48
Q

Atomic number is the number of ….

A

protons and electrons

49
Q

What is the octet rule

A

8 electrons in the outermost shell except hydrogen and helium

50
Q

What is covalent bonding

A

Sharing of a pair of electrons between two
non-metals.

51
Q

what are ions

A

Ions are molecules with a charge due to the difference of electrons.

52
Q

single bond vs double bond

A

single bond is the sharing of one electron between each other while a double bond is the sharing of two electrons between each other.

53
Q

An ion is formed when

A

an element loses or gains an electron

54
Q

what shows the number of orbits

A

period

55
Q

atomic mass is

A

protons + neutrons

Biology gr12 (9 decks)

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