Module 2 Flashcards

1
Q

Do electrons repel each other?

A

yes!

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2
Q

What makes most of an atom’s mass?

A

protons and neutrons

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3
Q

Are protons attracted to a neutron?

A

no

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4
Q

What compromises almost 100% of an atom’s volume?

A

The electron cloud

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5
Q

What determines the identity of an atom ?

A

The number of protons in the nucleus

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6
Q

if an element has 12 neutrons, can we figure out what it is?

A

no bc its based on protons

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7
Q

if calcium has a mass number of 42 how many neutrons?

A

22

40 - 20 = 22 (subtract the protons from mass # to get neutrons - remember it is a neutral and stable atom)

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8
Q

Sodium (Na) has a mass number of 23. How many protons, neutrons and electrons does this neutral sodium atom have?

A

11, 12, 11

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9
Q

Silver (Ag) has a mass number of 107. How many protons, neutrons and electrons does this neutral silver atom have?

A

47, 60, 47

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10
Q

An neutral atom has 33 electrons. Which element is it?

A

arsenic

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11
Q

How many neutrons are in an iron (Fe) atom that has a mass number of 56?

A

30

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12
Q

What are the number of protons, neutrons and electrons in the following isotope?

89 38Sr

A

38 protons, 51 neutrons, 38 electrons,

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13
Q

What are the number of protons, neutrons and electrons in the following isotope?

5224Cr

A

24, 28, 24

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14
Q

what is an isotope?

A

An isotope is a variant of a particular chemical element that has the same number of protons in its nucleus but a different number of neutrons. This means that isotopes of an element have the same atomic number (which defines the element) but different mass numbers.

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15
Q

What is the atomic symbol for the isotope that has 15 protons and 16 neutrons?

A

31 15 P

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16
Q

What is the atomic symbol for the isotope that has 35 protons and 45 neutrons?

17
Q

What is the atomic symbol for a mercury atom with 122 neutrons?

18
Q

Two isotopes of gallium are naturally occurring with 6931Ga at 60.11% (68.93 amu) and 7131Ga at 39.89% (70.92 amu). Calculate the atomic mass for gallium using the weighted average mass method.

19
Q

Two isotopes of rubidium occur naturally with 8537Rb at 72.17% (84.91 amu) and 8737Rb at 27.83% (86.91 amu). Calculate the atomic mass for rubidium using the weighted average mass method.

20
Q

What are alkali metals?

A

group 1a
very reactive, malleable, ductile
can explode when expose to water
one loose electron

21
Q

What are alkaline earth metals?

A

group 2
low electron affinity and electronegativity
two electrons in the outer shell
smaller atomic radius than alkali metals
readily form divalent cations

22
Q

Transitions metals, what are they ?

A

group 3 - 12
fairly unreactive, malleable
high melting and boiling points
low ionization energies

23
Q

What are halogens?

A

has very high electronegativities
seven valence electrons
highly reactive with alkali and alkaline earth metals
low ionization energies

24
Q

what are mettaloids ?

A

properties of non metals and metals
silvery mettalic
semi conductors
solid at room temperature

25
Q

Give the symbol of the element described by the following:

group 14, period 3

26
Q

Give the symbol of the element described by the following:

an alkali metal in period 3

27
Q

Which atom in the pair is larger? Na or Cl

28
Q

Which atom in the pair is larger? Na or Rb

29
Q

Place the elements in order of decreasing atomic size:

Cl, I, Br

30
Q

Which group on the periodic table are colourful and reactive non-metals?

31
Q

Which group on the periodic table are highly reactive, silvery, soft metals?

32
Q

Which group on the periodic table are chemically inert, colourless gases?

33
Q

What is the maximum electrons that can occupy the 4th shell?

34
Q

What is the maximum electrons that can occupy the 3d subshell?

35
Q

What is the maximum electrons that can occupy the 4f subshell?

36
Q

What is the maximum electrons that can occupy the 2p subshell?