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Quizzes > High School Quizzes > Science

Georgia EOC Physical Science Periodic Table Practice Quiz

Sharpen periodic table mastery for exam success

Difficulty: Moderate
Grade: Grade 9
Study OutcomesCheat Sheet
Colorful paper art promoting Elemental Power-Up, a science quiz for middle school students.

The modern periodic table is arranged by increasing ______.
Atomic number
Atomic mass
Electronegativity
Density
The modern periodic table is organized by atomic number, which represents the number of protons in an atom's nucleus. This arrangement produces a systematic pattern in chemical properties.
Which group of elements is known for being highly unreactive?
Noble gases
Alkali metals
Halogens
Transition metals
Noble gases have full valence electron shells, making them very stable and unreactive. Their complete outer electron configuration minimizes their tendency to engage in chemical reactions.
Which element is represented by the symbol 'O'?
Oxygen
Gold
Osmium
Oganesson
The symbol 'O' stands for oxygen, a nonmetal essential for most life processes. It is one of the most abundant elements on Earth and plays a key role in sustaining combustion and respiration.
Which of the following is a metal?
Sodium
Oxygen
Chlorine
Carbon
Sodium is classified as an alkali metal and exhibits metallic properties such as conductivity and malleability. In contrast, oxygen, chlorine, and carbon are nonmetals or metalloids.
What is the name of the horizontal rows in the periodic table?
Periods
Groups
Families
Blocks
The horizontal rows in the periodic table are called periods. They represent a recurring pattern of chemical properties as the elements increase in atomic number.
Which periodic trend describes the tendency of an atom to attract electrons in a chemical bond?
Electronegativity
Atomic radius
Ionization energy
Electron affinity
Electronegativity is the measure of an atom's ability to attract and hold electrons in a chemical bond. This trend is crucial for predicting the polarity and behavior of chemical bonds.
What trend is observed for atomic radius as you move down a group in the periodic table?
Atomic radius increases
Atomic radius decreases
Atomic radius remains constant
Atomic radius first decreases then increases
As you move down a group, additional electron shells are added to the atoms, making them larger. The increased distance between the nucleus and the outer electrons leads to an increase in atomic radius.
Which element has the electron configuration [Ne] 3s2 3p4?
Sulfur
Oxygen
Phosphorus
Chlorine
The electron configuration [Ne] 3s2 3p4 corresponds to an element with 16 electrons, which is sulfur. Recognizing electron configurations is key to identifying elements and understanding their chemical behavior.
In which group of the periodic table are the alkali metals found?
Group 1
Group 2
Group 17
Group 18
Alkali metals are located in Group 1 of the periodic table. Their single valence electron is responsible for their characteristic high reactivity.
What does the term 'periodic trend' refer to?
Variation in element properties across periods and groups
The pattern of element names
The history of element discovery
The order of atomic mass
Periodic trends are predictable variations in properties such as atomic radius, ionization energy, and electronegativity across the periodic table. These trends allow scientists to infer and compare the behavior of different elements.
Why do noble gases generally exhibit low chemical reactivity?
They have complete valence electron shells
They have high ionization energies
They have large atomic radii
They are located in the center of the periodic table
Noble gases possess complete valence electron shells, which make them stable and non-reactive. Their full electron configuration minimizes the need to gain or lose electrons, resulting in low chemical reactivity.
Which factor is primarily responsible for the decrease in ionization energy down a group?
Increased electron shielding
Increased nuclear charge
Decrease in atomic mass
Decrease in electron shielding
As you move down a group, additional electron shells create more electron shielding, which reduces the effective nuclear charge felt by the outer electrons. This decreased attraction makes it easier to remove an electron, lowering the ionization energy.
Which type of chemical bond is formed by the sharing of electrons between atoms?
Covalent bond
Ionic bond
Metallic bond
Hydrogen bond
A covalent bond is formed when atoms share electrons in order to achieve a stable electron configuration. This sharing typically results in the formation of strong bonds between nonmetal atoms.
How does periodicity influence the chemical properties of elements?
Elements in the same group exhibit similar chemical properties
Elements in the same period have identical properties
Properties randomly vary across the table
Chemical properties are independent of periodic trends
Elements in the same group have similar valence electron configurations, which results in similar chemical properties and reactivity. This periodicity is a cornerstone of the periodic table's design.
Which element is considered a metalloid and is located near the dividing line between metals and nonmetals?
Silicon
Sodium
Iron
Helium
Silicon is classified as a metalloid because it has properties of both metals and nonmetals. Its intermediate electron conductivity makes it especially important in the electronics industry.
Given that electronegativity increases across a period and decreases down a group, which element is expected to have a higher electronegativity: fluorine or chlorine?
Fluorine
Chlorine
Both are equal
Neither have notable electronegativity
Fluorine is situated at the top of Group 17 and, due to its small atomic size and minimal electron shielding, it exhibits the highest electronegativity. This makes fluorine exceptionally effective at attracting electrons within chemical bonds.
If an element in Period 3 has a valence electron configuration of 3s2 3p1, to which group does it belong and what is one of its characteristic chemical behaviors?
Group 13; it tends to form +3 ions
Group 14; it generally forms covalent bonds
Group 11; it shows low reactivity
Group 18; it is inert
An electron configuration of 3s2 3p1 indicates three valence electrons, placing the element in Group 13. Elements in this group typically lose these three electrons to form +3 ions, which is a key aspect of their chemical behavior.
How does the concept of effective nuclear charge help explain the trend in atomic radii across a period?
It shows that increased nuclear charge pulls electrons closer, decreasing atomic radii
It indicates that more protons always increase the size of an atom
It suggests that added electrons have no effect on atomic size
It reveals that increased effective nuclear charge always results in larger atoms
Effective nuclear charge is the net positive charge felt by electrons after accounting for shielding. As the nuclear charge increases across a period, it pulls electrons closer, thereby reducing the atomic radius.
Considering periodic trends, which pair of elements is expected to have the largest difference in first ionization energy?
Helium and Francium
Lithium and Beryllium
Carbon and Nitrogen
Oxygen and Fluorine
Helium possesses a very high ionization energy due to its small size and strong nuclear attraction, while Francium has one of the lowest ionization energies because of its large atomic radius and increased electron shielding. This pair, therefore, exhibits a significant difference in their tendencies to lose electrons.
How does the structure of the periodic table facilitate predictions about chemical reactivity?
Similar groups indicate similar reactivity due to analogous valence electron configurations
The horizontal rows show that all elements react identically
The position provides no clues about reactivity
The structure only indicates atomic mass
The periodic table arranges elements into groups and periods based on their electron configurations. Elements within the same group have similar valence electron arrangements, which leads to comparable chemical reactivity and behavior.
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Study Outcomes

  1. Understand key periodic trends such as electronegativity, ionization energy, and atomic radius.
  2. Analyze the organization of the periodic table to identify element groups and periods.
  3. Apply element classification concepts to predict chemical and physical properties.
  4. Evaluate how periodic trends influence element reactivity and behavior.
  5. Interpret periodic table data to support conclusions about elemental properties.

GA EOC Physical Science Periodic Table Cheat Sheet

  1. Periodic table organization - Think of the periodic table as a grand party where elements line up in periods (rows) and groups (columns). Those in the same group share similar chemical vibes because they've got the same number of valence electrons. It's your go‑to roadmap for predicting how elements behave when they mingle or clash! ThoughtCo
  2. Atomic radius trends - As you slide down a group, atomic radius balloons because each new row adds an electron shell, making the element look bigger. But move left to right across a period and the radius shrinks; the growing nuclear charge tugs electrons closer, tightening that atomic hug. It's like pulling a rubber band tighter with each proton you add! Learning Box
  3. Ionization energy - Ionization energy is the "tug‑of‑war" strength needed to yank an electron away from an atom. It generally climbs across a period because atoms hold their electrons more fiercely, and drops down a group as atoms get larger and electrons sit farther out. Master this trend and you'll predict who's easy to ionize and who's a stubborn holdout! Save My Exams
  4. Electronegativity - Electronegativity measures how badly an atom wants electrons in a bond - like a chemistry popularity contest. It rises across a period as atoms become more electron‑hungry, and falls down a group when the grip on outer electrons loosens. This trend dictates bond polarity, so it's key for predicting molecular drama! Learning Box
  5. Electron affinity - Electron affinity tells you the energy change when an atom gains an electron - negative values mean the atom can't wait to take on more. Overall it gets more negative across a period since atoms want to complete their valence shell, though a few quirky exceptions pop up. Understanding this helps you foresee which elements love extra electrons and which are more "meh." Learning Box
  6. Metallic character - Metallic character is all about how readily an element loses electrons to form positive ions - basically, how "metal‑like" it is. It fades across a period (elements get less willing to part with electrons) and shines brighter down a group (atoms get bigger and more generous). Use this trend to decide who's a classic metal and who's playing for Team Nonmetal! Learning Box
  7. Effective nuclear charge (Zeff) - Zeff is the net positive pull an atom's nucleus exerts on its valence electrons, calculated roughly as Z - S (atomic number minus shielding electrons). It climbs across a period, tightening the nucleus's grip and shrinking atomic size. Grasping Zeff helps you decode why trends like radius and ionization energy behave the way they do! Learning Box
  8. Metal, nonmetal, metalloid classification - Elements fall into three squads: metals (malleable, conductive, electron‑donors), nonmetals (often insulative, varied in form), and metalloids (mixed traits, the chemistry's middle children). Their spot on the table spells out their identity and hints at their chemical career path. Knowing the lineup is like having backstage passes to the element concert! ThoughtCo
  9. Transition metals - Sitting in groups 3 - 12, transition metals are the chemistry chameleons with multiple oxidation states and dazzling colored compounds. Their d‑orbitals let electrons hop around, producing vibrant hues in solutions and minerals. These shape‑shifters are crucial catalysts and heroes in industrial chemistry! ThoughtCo
  10. Noble gases - Noble gases in group 18 boast full valence shells, making them the cool, unreactive VIPs of the table. They're so stable you'll find them lighting up neon signs or chilling in high‑tech lasers rather than bonding with others. Remember - no free electrons needed, they've already got the perfect party mix! ThoughtCo
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