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chemistry 11 > unit 1 > Flashcards

unit 1 Flashcards

1
Q

what is an isotope

A

-atoms of an element that have same number of protons (atomic number) but different number of neutrons (atomic mass)

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2
Q

how is an isotope written

A

carbon - 14

or

35 —> atomic mass
Cl
17 —> atomic number

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3
Q

what is isotopic abundance

A

-the percentage of a given isotope in a sample of an element
-percents of isotopes of same element add to 100%

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4
Q

what is a radioisotope

A

-isotopes which can decay and emit radiation as their nucleus

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5
Q

what is the formula for finding the atomic mass of an isotope

A

atomic mass =
% abundance of isotope 1(mass of isotope 1)
+
% abundance of isotope 2(mass of isotope 2)

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6
Q

what are the trends in a group in the periodic table

A

-have same chemical properties and reactivity bc same number of valence electrons
-for metals reactivity increases moving down a group
-for non-metals reactivity decreases moving down a group

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7
Q

what are the rules to follow for atoms containing many electrons

A

1) electrons always occupy the lowest possible energy level (orbital)
2) there is a maximum number of electrons in each level
—> the number is given by 2n^2 where n is the principle quantum number

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8
Q

what was Mendeleev’s periodic table

A

-chemists who published the first periodic law
-elements arrange in order of increasing atomic mass show a periodic recurrence of properties

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9
Q

how is the modern periodic table organized

A

-after Mendeleev the periodic law was revised
-when elements are strange in order of increasing atomic numbers their properties show a periodic recurrence and gradual change

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10
Q

what is atomic radius

A

-a measurement of the size of an atom
-atomic radii decrease from left to right across a period

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11
Q

what is nuclear charge

A

-charge in nucleus
-more protons in nucleus = stronger charge that pulls electrons in and creates smaller radius

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12
Q

What are IONIC properties?

A

-high melting point
-conduct electricity when liquid or in solution

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13
Q

What are the MOLECULAR properties?

A

-low melting points
-do not conduct
-atoms shared equally —> molecule non-polar
-atoms not shared —>molecular polar

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14
Q

What did The Alchemist do?

A

-transfer common metals to gold
-explored matter of nature
-searched for “elixir of life” and philosophers stone
-made lab glassware, equipment, procedures, and processes that are still used today

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15
Q

What was Daltons theory?

A

-all matter is made up of tiny invisible particles called atoms
-all atoms of an element are identical
-atoms of different elements are different
-atoms are rearranged to form new substances in chemical reactions but cannot be created or destroyed

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16
Q

What did Thomson discover?

A

-discovered the electron
-proposed that they are negatively charged small part of an atom
-made plum pudding model

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17
Q

What did Rutherford do?

A

-aimed alpha particles at a sheet of gold foil and measured how much the foil deflected particles
-guessed that they would go through
-was proven wrong because some deflected (they hit protons)
-concluded that atoms have a small, dense, positively charged, central nucleus

18
Q

What did Chadwick discover

A

nuclei contain neutral particles known as NEUTRONS

19
Q

What did Bohr discover?

A

-electrons are in orbits of differing energy (energy levels)
-electrons start at ground level but can absorb energy and go to excited state
-after being excited they release energy and this energy occupies a portion of the electromagnetic spectrum
-different energy levels have different numbers of electrons
-the bohr model only works for simple atoms

20
Q

what is ionic radius

A

-measure of the size of an atom
-metal ions get smaller because they lose electrons
-non metals get larger bc they gain electrons

21
Q

what is ionization energy

A

-amount of energy required to move an electron from an atom
-energy varies depending on which electron is being bc removed (closer to nucleus = more energy needed to remove)

22
Q

what is first ionization energy

A

-amount of energy required to remove most weakly held electron

23
Q

what is the trend in ionization energy

A

-increases going up a group
-increases across a period
—> metals want to give away electrons to be stable so it requires less energy

24
Q

what is electron affinity

A

energy charge that occurs when an electron is accepted by an atom

25
Q

what is electronegativity

A

-number that describes availability of an atom when bonded to an electron

26
Q

what is the trend in electronegativity

A

decreases going down a group and increases across a period

27
Q

what is compound formation

A

-when valence electrons make a new arrangement that has less energy than their previous arrangement

28
Q

how do you show an ionic bond

A

using louis dot diagrams

29
Q

what is a formula unit

A

simplest whole number ratio of atoms and ions of an element in an ionic compound
ex. NaCl has 1:1 ratio

30
Q

what is a crystal lattice

A

a regular ordered arrangement of atoms, ions, or molecules

31
Q

what are the three types of covalent bonds

A

-single (one pair of electrons share)
-double (two pairs of electrons shared)
-triple (three pairs of electrons shared)

32
Q

what is a lone pair

A

electrons not involved in bonding

33
Q

what is electrical conductivity

A

-the ability of material to allow electricity to flow through it
-solutions that conduct electricity are called electrolytes

34
Q

what are the rules for drawing structural diagrams

A

-central element - element with highest bonding capacity or lowest electronegativity
-arrange elements
-count total # of valence electrons
-place a pair of electrons between each element
-place lone pairs around surrounding elements (not central)
-if more electrons left over put them around central
-make sure all elements are happy, if not use co-ordinate covalent

35
Q

what is a polyatomic ion

A

-it is an ion with a charge
-positive = less electrons, negative = more electrons

36
Q

how do you draw a structural diagram for a polyatomic ion

A

-do all same steps as before
-when counting valence electrons add one for each unit of negative charge or subtract one for each unit of positive charge
-draw brackets around structure with its charge outside

37
Q

what are the three types of bonds

A

-ionic
-polar
-non-polar

38
Q

what is the electronegative of an ionic compound

A

-1.7 or more

39
Q

what are polar covalent bonds

A

-when electrons are not shared equally
-difference between 0.39 and 1.69
-on is partially positive and the other is partially negative (the higher electronegativity is negative)
-draw arrow to show which element is the hog

40
Q

what is a non-polar covalent bond

A

-electrons shared equally
-difference between 0 and 0.39
-shared equally so no charge or arrow

chemistry 11 (2 decks)

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